Slide 1

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 2

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 3

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 4

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 5

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 6

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 7

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 8

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 9

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 10

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 11

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 12

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 13

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 14

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 15

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 16

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 17

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 18

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 19

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 20

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 21

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 22

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 23

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 24

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 25

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 26

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 27

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 28

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 29

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 30

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 31

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 32

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 33

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 34

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 35

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 36

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 37

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 38

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 39

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 40

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 41

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 42

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 43

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 44

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 45

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 46

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 47

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 48

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 49

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 50

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 51

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 52

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 53

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 54

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 55

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 56

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 57

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 58

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 59

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 60

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 61

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 62

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 63

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 64

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 65

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 66

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 67

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 68

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 69

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 70

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 71

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 72

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 73

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 74

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 75

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 76

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 77

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 78

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 79

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 80

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 81

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 82

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 83

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 84

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 85

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 86

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 87

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 88

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 89

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 90

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 91

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 92

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 93

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 94

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 95

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 96

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 97

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 98

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 99

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 100

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 101

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 102

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 103

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 104

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 105

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 106

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 107

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 108

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 109

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 110

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 111

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 112

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 113

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 114

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 115

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.


Slide 116

TAKS Objective 4
Coach Smith
Waco High Chemistry
2006-2007

Objective 4

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.

Mass = 40 g

Volume = 20 mL

Density = Mass / Volume

D=m/v

1. The picture shows a cube that contains 20 mL of a
solution. The solution has a mass of 40 grams.
What is the density in g/ml of this solution? Record
and bubble in your answer on the answer
document.
40 g / 20 mL = 2.0 g / mL

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
F. Gain mass
G. Shrink
H. Increase in solute content
J. Start to vibrate.

Objective 4

95% water
98% water

Permeable to
water only

2. The picture shows a cell model and the solutions
associated with it. In this situation the cell model
will –
G. Shrink

Black-and-White Negatives

Objective 1 & 4

Before digital cameras were available, photographs could be made only with
cameras that used photographic film. These cameras are still in use today.
Photographic film contains a light-sensitive layer of chemicals. These chemicals
are silver halide granules. As light rays travel through a camera lens, they bend and are
focused onto the photographic film. When exposed to light, the silver halide granules
are activated in different amounts depending on the intensity of the light that strikes
them. This forms a photographic image on the film.
After the pictures are taken, the exposed film is processed in a laboratory. The film
is placed in a solution that reacts chemically with the silver halide granules, forming
black metallic silver. The black silver is thickest in the areas of the film exposed to the
most intense light and thinnest in the areas exposed to the least intense light.
After a roll of film is processed, it is called a negative. This is because it contains
negative images of the pictures that were taken. When light is projected through the
negative onto photosensitive paper, the areas with the thickest silver become the
lightest, and the areas with the thinnest silver become the darkest.
The diagram shows both a negative image and a positive image of a tree. The
negative image represents an image on the negative, and the positive image represents
the same image on photo paper.
Negative Image

Positive Image

Objective 4

3. In photography, which of these is an example
of a chemical change?
A.
B.
C.
D.

Light being refracted by a camera lens.
Adjusting a lens to focus light.
Halide granules being activated by light.
Allowing a certain wavelength of light
into the camera.

3. In photography, which of these is an example
of a chemical change?

C. Halide granules being activated by light.

Objective 4

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

Silver Bromide
Group 17 Elements are also called the Halogens,
which make (halides) when in compounds.

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?
F. Group 4
G. Group 5
H. Group 10
J. Group 17

4. Silver bromide is a type of halide.
Elements from which group in the periodic
table are necessary to form halide
compounds?

J. Group 17

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?
A. Q
B. R
C. S
D. T

Objective 4

5. Elements found in which shaded area of this periodic
table undergo the fewest chemical reactions?

D. T

Objective 4

__Ca(C2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?
F.
G.
H.
J.

3, 3, 1, 2
6, 1, 1, 3
3, 2, 1, 6
6, 2, 1, 6

2
6
3
1
__Ca(C
2H3O2)2 + __K3PO4  __Ca3(PO4)2 + __KC2H3O2
# of
Reactants
Step 1: Count the
number of
each element.
Step 2: Use Coefficients
to balance the
equation.

# of
Products

1

Ca

3

12 4
18 6
20 12 8

C

2

12

H

3

18

O

6

3

K

10 20
1 6

2

1

P

2

3

6. Which set of coefficients balances the equation?

H. 3, 2, 1, 6

Objective 4

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –
A.
B.
C.
D.

Melted
Boiled
Reacted chemically
Become hydrated

7. A sugar cube in a test tube is heated over a
Bunsen burner. The sugar cube turns black
and has less mass than before it was
heated. These changes occur because the
sugar has –

C. Reacted chemically

Objective 4

8. The structure of pure water makes it a good –
F.
G.
H.
J.

Solvent
Catalyst
Conductor
Nutrient

8. The structure of pure water makes it a good –
F. Solvent

Objective 4

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?
A.
B.
C.
D.

1:1
4:1
1:8
1:50

2.50
20.0

=

1
8

Initial volume = 2.50 L
Mass = 1 g

Final volume = 20.0 L
Mass = 1 g

9. The diagram represents helium gas expanding to fill a large
container. What is the ratio of the helium gas’s density at the
final volume to its density at the initial volume?

C. 1:8

2.50
20.0

=

1
8

Objective 4

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

Elements in the same group have similar
characteristics.

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –
F.
G.
H.
J.

Hydrogen
Silicon
Helium
Sulfur

10. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of –

J. Sulfur

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.
A. Heating the reactants to ensure the
reaction occurs in a gaseous state.
B. Subtracting the mass of the gas from the
mass of the solid and liquid products.
C. Mixing the reactants and measuring their
total mass.
D. Trapping the gas and measuring its mass.

Objective 4

11. Which of these would support the idea that
mass is conserved in a reaction that produces
a gas as a product.

D. Trapping the gas and measuring its mass.

Objective 4

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?
F.
G.
H.
J.

Al + O2  Al2O3
2Al + 2O2  2Al2O3
2Al + 3O2  5Al2O3
4Al + 3O2  2Al2O3

4 Al + __
3 O2  __
2 Al2O3
__
# of
Reactants
Step 1: Count the
number of
each element.

# of
Products

4

1

Al

2

6

2

O

3

4
6

Step 2: Use Coefficients
to balance the
equation.

12. Aluminum metal and oxygen gas combine to produce
aluminum oxide (Al2O3). Which of these is the balanced
chemical equation?

J. 4Al + 3O2  2Al2O3

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
A.
B.
C.
D.

Solution 1
Solution 2
Solution 3
Solution 4

Objective 4

Properties of Some Solutions
Electrical
Color of Litmus
Original Color of
Solution Conductivity
Paper After Dipping
Litmus Paper
of Solution
in Solution

pH

1

Very High

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very High

Blue

Red

2.0

13. The table shows data from an investigation designed to
find a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

D. Solution 4

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

F.
G.
H.
J.

Sodium
Neon
Magnesium
Argon

Periods show the Energy Levels
Groups show the Number of Valence Electrons

Objective 4

Energy Level

1

2

3

Electrons

2

8

8

14. According to the periodic table and the
information above, which element has this
electron configuration?

J. Argon

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?

A. S
B. Mg
C. F
D. Rb

Group 2 Elements tend to lose two electrons when
forming chemical bonds, giving them a -2 charge.

Objective 4

15. According to the periodic table, which of these
elements will form an ion with a -2 charge?
B. Mg

Objective 4

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –
F. Increases the moisture of the sugar.
G. Decreases the volume of molasses.
H. Increases the density of sugar.
J. Decreases the viscosity of molasses.

16. Brown sugar consists of crystals of white sugar
coated with molasses. If brown sugar hardens, it
can be softened by heating. The most likely
reason brown sugar softens when heated is that
heat –

J. Decreases the viscosity of molasses.

Objective 4

17. As the viscosity of a liquid increases, the liquid –
A. Conducts electricity
B. Pours more slowly
C. Evaporates more quickly
D. Forms a precipitate

Objective 4

17. As the viscosity of a liquid increases, the liquid –
B. Pours more slowly

Objective 4

18. Dissolving salt in water increases the conductivity
of the solution because the –
F. Salt gives the solution a net negative charge.
G.Salt ions bond with the available water
molecules.
H. Solution has an increase in kinetic energy.
J. Concentration of ions in the solution increases.

18. Dissolving salt in water increases the conductivity
of the solution because the –

J. Concentration of ions in the solution increases.

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
A. Ultraviolet light
B. Air pressure
C. Gravitational force
D. Thermal energy

Objective 4

19. Water normally boils at 100°C at sea level and at
97°C on a North American mountaintop. This
difference in boiling points can be explained by
the difference between the locations’ –
B. Air pressure

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –
F.
G.
H.
J.

Acidity
Clarity
Solubility
Density

Objective 4

20. The buoyant force that a fluid exerts on
objects is increased when there is an
increase in the fluid’s –

J. Density

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –
A.
B.
C.
D.

Group 2 elements are electrically neutral.
Group 2 elements have two valence electrons.
Group 2 elements contain neutrons in the nucleus.
Group 2 contains more elements than other groups.

Objective 4

Examples
of Group 2
elements

Examples
of Group 16
Elements

2 Mg

+

O2

 2 MgO

Ca

+

S



CaS

21. The ionic compounds that result from combining Group 2
and Group 16 elements have a 1:1 ratio because –

B. Group 2 elements have two valence electrons.

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
F. Massive
G. Dense
H. Viscous
J. Soluble

Objective 4

22. The picture shows the results of pouring a blue
liquid into a clear liquid and allowing the mixture to
settle for 25 minutes. Compared to the clear
liquid, the blue liquid is more –
G. Dense

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –
A. Have differences in reactivity
B. Are able to bond with oxygen
C. Vary in solubility
D. Exist in different phases

Objective 4

23. Compounds with the same chemical composition
may have different densities because they –

D. Exist in different phases

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?
F. 4OH (aq)
G. CH4(g)
H. H2O2(g)
J. 2H2O(g)

Objective 4

2C2H2 + 5O2  4CO2 + 2H2O
# of
# of
Reactants
Products
4
C
4
4
H
0 4
10
O
8 10

24. Which additional product balances this reaction?

J. 2H2O(g)

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –
A. Increases the pressure of the river water.
B. Increases the pH value of the river water.
C. Decreases sediment solubility in the river
water.
D. Decreases the dissolved oxygen in the
river water.

Objective 4

25. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water temperature –

D. Decreases the dissolved oxygen in the
river water.

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F.
G.
H.
J.

Q
R
S
T

Objective 4

Liquid

Description

Density
(g/mL)

Boiling Point
(°C)

Q

Nonflammable colorless
compound

1.62

59.5

R

Flammable colorless
compound

0.71

34.6

S

Yellow mixture with strong
odor

0.73

160.4

T

Viscous pale-yellow oil

0.93

300.0

26. The table shows properties of four liquids that are
insoluble in water. If the four liquids are poured into an
Erlenmeyer flask containing water, which liquid will form
a layer below the water?
F. Q

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

A. Its transparency in light
B. Its electrical conductivity
C. Its physical state of matter
D. Its molecular arrangement

Objective 4

27. Which characteristic of water best explains its
ability to dissolve a great variety of materials?

D. Its molecular arrangement

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?

0 Temperature 100
(°C)

0 Temperature 100
(°C)

D

0 Temperature 100
(°C)

60

Solubility
(g/100 mL)

C

60

Solubility
(g/100 mL)

B

60

Solubility
(g/100 mL)

Solubility
(g/100 mL)

A

60

0 Temperature 100
(°C)

Group Temperature (°C) Solubility (g/100 mL)
A
0
28
B
10
31
C
20
34
D
30
37
E
40
40
F
60
45
G
80
51
H
90
54
I
100
56

Objective 4

28. Nine groups of students dissolved as much potassium chloride
as possible in water. Each group used 100 mL of water heated to
a different temperature. Which graph shows the relationship
between solubility and temperature for potassium chloride?
Solubility
(g/100 mL)

D

60

0 Temperature 100
(°C)

Objective 4

29. Which of these elements is most likely to
donate one electron?

A. Be
B. Cs
C. Rn
D. He

Objective 4

Elements in Group 1 have only 1 valence electron, which
they lose when bonding.

Objective 4

29. Which of these elements is most likely to
donate one electron?
B. Cs

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

F. Actinium
G. Curium
H. Radium
J. Helium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

30. Alpha particles are one type of radioactivity.
These particles have a nucleus of two protons
and two neutrons but have no orbital electrons.
Based on this information, it can be inferred that
alpha particles are positive ions of the element –

J. Helium

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
A. Silicon
B. Carbon
C. Magnesium
D. Calcium

Objective 4

The atomic number of any element is the number of protons
in an atom of that element.

Objective 4

31. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is
a form of the element –
B. Carbon

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?
F. Group 6
G. Group 12
H. Group 14
J. Group 18

Objective 4

Group 14 (4A) has 4 valence electrons, which it can share in
a covalent bond with 2 oxygen atoms.

Objective 4

O=X=O
32. The model above shows how an unidentified
element, X, forms covalent bonds with oxygen.
In which group on the periodic table does
Element X most likely belong?

H. Group 14

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

A.
B.
C.
D.

W
X
Y
Z

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
Z product mixture, and the combination is
ground into a powder. The result is
portland cement.

Objective 4

How Portland Cement is Made

33. Portland cement is used
to make concrete, a very
common construction
material. Which step in
the production of
portland cement causes
a chemical change?

C. Y

Raw Materials:
Limestone
Clay/shale
(CaCO3)
(SiO2, Al2O3, Fe2O3)

W

Raw materials are dug from a quarry
and crushed.

X

Crushed materials are mixed
and ground together.

Y

The mixture is heated in an oven.
(O2)
Product mixture:
Ca3SiO5, Ca2SiO4, Ca3Al2O6, Ca2Fe2O5

Gypsum (CaSO4) is added to the
product mixture, and the
Z
combination is ground into a powder.
The result is portland cement.

Objective 4

Gas Sylvestre
Early alchemists were able to produce various kinds of gases by mixing
different substances together. However, it was not until the early 1600s that a
Belgian physician, J. B. van Helmont, first used the term gas.
Van Helmont concentrated his study on a gas he obtained from the
burning of wood. He called this substance gas sylvestre, which means “gas
from wood.” He demonstrated that gas sylvestre also formed when limestone
reacted with an acid solution. Van Helmont determined that the gas was
denser than air and occurred naturally in the lower chambers of the Grotto
del Cane, a cave in Italy. He noticed that the atmosphere in the lower cave did
not support animal life. He also observed that the process of fermentation
produced gas sylvestre. Today gas sylvestre is known by a more familiar
name—carbon dioxide.

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.
G. Solid carbon dioxide becomes a gas at
room temperature.
H. Limestone combined with sand results in a
mixture.
J. Diluting an acid with water produces a
solution

Objective 4

34. Which of the following describes a chemical
change that J.B. van Helmont could have
observed?
F. Limestone combined with an acid produces
a gas.

Reaction of Copper with Sulfur
Mass of Cu before reaction:
Mass of S before reaction:

3.17 g
2.93 g

Mass of CuS formed
Mass of unreacted S:

4.78 g
?g

Objective 4

Mass of Reactants = Mass of Products
3.17 + 2.93 = 6.10
4.78 + ? = 6.10
- 4.78
Answer = 1.32

35. Copper (Cu) and sulfur (S) were heated in a covered
container. After the reaction was complete, the unreacted
sulfur was removed. The table contains the results of the
investigation. How much sulfur, in grams, failed to react
with the copper? Record and bubble in your answer to
the nearest hundredth on the answer document.

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

C

B

D

Objective 4

36. In which model of the periodic table does the
shaded area show the location of elements that
require the least energy to lose one electron?

A

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?
A. Chemical stability
B. High polarity
C. Low melting point
D. High freezing point

Objective 4

37. The graph shows the concentration of ions found
in the water of the Dead Sea. Which property of
water is responsible for the dissociation of salts
that produces the ion concentrations shown in
the graph?

B. High polarity

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
F. Freezing the water
G. Separating the water into its elements.
H. Calculating the water’s density
J. Dissolving sugar in the water

Objective 4

38. Which process best demonstrates a chemical
change in distilled water?
G. Separating the water into its elements.

Objective 4

39. Which of these describes a chemical change?
A. Frost disappears from a window in the
morning.
B. A decrease in temperature reduces the
volume of a gas.
C. Soot is formed as a candle burns.
D. A cup of hot tea cools down.

Objective 4

39. Which of these describes a chemical change?

C. Soot is formed as a candle burns.

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F.
G.
H.
J.

0°C
10°C
30°C
40°C

MTBE Solubility
Temperature
(°C)
0
9.7
19.8
29.6
39.3
48.6

Objective 4

Solubility
(grams per liter)
83
51
42
31
25
19

40. MTBE is a gasoline additive that has entered some
groundwater supplies. According to the table above,
which of the following water temperatures would allow
79 grams of MTBE to dissolve in 1 liter of water?
F. 0°C

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?
A. Freezing water cracking limestone
B. Flowing water eroding a limestone riverbed
C. Acid rain forming puddles on limestone
D. Coastal waves dissolving limestone
sediments.

Objective 4

41. Limestone is a sedimentary rock consisting
mostly of calcium carbonate (CaCO3). Which
process is most likely to cause a chemical
change to limestone?

C. Acid rain forming puddles on limestone

Objective 5

m
d

v

400
= 0.5
800

42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
F.
G.
H.
J.

0.30 g/cm3
0.50 g/cm3
0.80 g/cm3
1.30 g/cm3

Density =

Mass
Volume

Objective 5

d = 0.5
42. A 500 mL quantity of vanilla ice cream has a
mass of 400 grams. The manufacturer then
bubbles air into the ice cream so that its
volume increases by 300 mL. What is the
ice cream’s approximate final density?
Density =

G. 0.50 g/cm3

Mass
Volume

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

A. Sodium
B. Potassium
C. Strontium
D. Rubidium

Elements in the same group have
similar characteristics.

Objective 4

43. Calcium ions play an important role in the
function of neurons in the brain. Elements that
are chemically similar to calcium can interfere
with the function of neurons. Which of the
following is the most likely to imitate calcium’s
role in the function of neurons?

C. Strontium

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

F. Is a physical change.
G. Involves an energy-to-matter
conversion.
H. Decreases the density of the metal.
J. Involves metal bonding with other
atoms.

Objective 5

44. The mass of a rusty bicycle is found to be
slightly greater than the mass of the same
bicycle before it rusted. The change in mass
indicates that the rusting process –

J. Involves metal bonding with other
atoms.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.
B. Gravity rotates the oxygen atoms to face the moremassive sodium ions.
C. Hydrogen atoms create repulsive forces with chloride
ions.
D. Oxygen atoms from covalent bonds with sodium ions.

Objective 4

NaCl Crystal

Water Solution

45. The diagram on the right shows water molecules and ions
from an NaCl crystal. What is the most likely reason that
each water molecule is arranged so that the oxygen part of
the molecule faces a sodium ion?
A. The oxygen in a water molecule contains a partial
negative charge.

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –
F.
G.
H.
J.

Solution 1
Solution 2
Solution 3
Solution 4

Properties of Some Solutions
Electrical
Color of
Original Color of
Solution Conductivity
Litmus Paper After
Litmus Paper
of Solution
Dipping in Solution

Objective 5

pH

1

Very high

Red

Blue

10.0

2

Low

Blue

Red

6.5

3

Moderate

Red

Red

5.4

4

Very high

Blue

Red

2.0

46. The table shows data from an investigatin designed to find
a liquid solution that is both an acid and a strong
electrolyte. Based on the data, a solution that is both an
acid and a strong electrolyte is –

J. Solution 4

Objective 4

47. Water acts as a solvent of ionic compounds
because –
A. Water is a liquid over a wide range of
temperatures.
B. Water molecules are polar.
C. Water is found in three states of matter.
D. Water takes the shape of its container.

Objective 4

47. Water acts as a solvent of ionic compounds
because –

B. Water molecules are polar.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.
G. The rate of vibration of the molecules.
H. The kinds of dissolved substances
between the molecules.
J. The amount of energy the molecules
can absorb.

Objective 5

48. Which of these remains the same while
water molecules go through the water
cycle?
F. The ratio of oxygen to hydrogen in the
molecules.

Objective 4

Soap-Making Project
Materials:
125 mL cooking oil
100 mL H2O
10 g NaOH
Safety goggles
Apron
500 mL beaker
Stirring rod
Procedure:
• Measure and add 100 mL of H2O to 125 mL of cooking oil and mix
thoroughly.
• Carefully and slowly add 10 g of NaOH while stirring constantly.
• Stir until a thick paste forms.
• Pour the paste into a mold and let it sit for two days.
• Remove the solid bar from the mold.
Caution:
Keep this soap away from the face and eyes because traces of NaOH
may still be present on the soap bar. Use this soap for washing
floors and tools only.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?
A. Making grooves in the surface of the
thick paste.
B. Adding air bubbles to the thick paste.
C. Letting the thick paste sit for four days.
D. Chilling the mold filled with the thick
paste.

Objective 4

49. A bar of soap produced by this soapmaking process normally sinks to the
bottom of a container of water. Which of
these processes could cause the bar of
soap to float in water?

B. Adding air bubbles to the thick paste.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.
G. An apple being bitten
H. An ice cube being swallowed
J. Absorption of a water molecule.

Objective 5

50. Which of the following is an example of a
chemical change.
F. Combustion of gasoline.