Transcript S.O.L. Review

S.O.L. Review
Down to the wire!
What do you need to do now?
 Eat a good dinner, go to bed at a
decent hour.
 Be on time for school tomorrow.
 Eat a good breakfast and avoid
excess caffeine.
 I will be serving snacks in my room
from 8:15-8:50
 Your SOL is in the library at 9:05
What do I need to study?
 Review with your flashcards, but
remember they do not cover
everything
 Review the chapter summaries in
your textbook
 Look over your notes and old tests
 Look at the ppt on my website
 USA Test Preps & J-Labs ARE NOT
ENOUGH!!!!!
Gas Laws
P, V?
P, T?
V, T?
What law does this graph
represent?
Chemical or Physical Change?
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A banana turns brown
Water boils
Licking a lollipop
Baking bread
Soda explodes when you shake it up
Safety
 What do you do with waste chemicals?
 Where do you find information on a
chemical?
 What equipment protects you from
toxic vapors?
 Where does broken glass go?
 What do you do when you get
splashed with a chemical?
Name these chemicals!
 NaF
 sodium fluoride
 K2CO3
 potassium
carbonate
 MgCl2
 magnesium chloride
 Be(OH)2
 beryllium hydroxide
 Ca3(PO4)2
 calcium phosphate
 (NH4)2SO4
 ammonium sulfate
 Mn(NO3)3
 manganese (III)
nitrate
 FePO4
 iron (III) phosphate
Write these formulas!
 potassium fluoride
 KF
 ammonium nitrate
 NH4NO3
 magnesium iodide
 MgI2
 copper (II) sulfate
 CuSO4
 aluminum phosphate
 AlPO4
 lead (II) nitrate
 Pb(NO3)2
 cobalt (II) selenide
 CoSe
 silver cyanide
 AgCN
 copper (II) carbonate
 CuCO3
 iron (II) oxide
 FeO
These are covalent, why?
 SiF4
 silicon tetrafluoride
 N2S3
 dinitrogen trisulfide
 HBr
 hydrogen bromide (or hydrobromic
acid)
 Br2
 bromine
Write these covalent compounds?
 diboron hexahydride
 B2H6
 nitrogen tribromide
 NBr3
 sulfur hexafluoride
 SF6
 diphosphorus pentoxide
 P2O5
What is the empirical formula?
 C2H4O2
 CH2O
 methane
 CH4
 C6H12O6
 CH2O
What do these look like?
 carbon disulfide
 CS2 is linear and non-polar
 boron trifluoride
 BF3 is trigonal planar and non-polar
 difluoromethane
 CH2F2 is tetrahedral and polar
Conversions . . . YEA!
 30 grams of H3PO4
 0.31 moles
 25 grams of HF
 1.25 moles
 110 grams of NaHCO3
 1.31 moles
 1.1 grams of FeCl3
 0.0068 moles
Moles to mass . . .
 4 moles of Cu(CN)2
 462 grams
 5.6 moles of C6H6
 436.8 grams
 21.3 moles of BaCO3
 4202.5 grams
 1.2 moles of (NH4)3PO3
 159.6 grams
Moles  gas volume . . .
 25 Liters of O2
 1.12 moles
 10 moles of N2
 224 L
 1.0 x 105 Liters NH3
 4460 moles
 2.35 x 10-2 moles H2O(g)
 0.527 L
Percent Error
 If you measured 23 out of 90
 74.4% error
 If you measured 78 out of 85
 8.23% error
 If you start with 100g but only
recover 43%.
 57% error
Balancing Equations
 Balance equations because of the Law of
Conservation of Matter: the mass of the
reactants = mass of products
__N2 + __H2  __NH3
__C6H12O6 + __O2 __H2O + __CO2
__Ca3(PO4)2 + __ZnCl2  __CaCl2 + __Zn3(PO4)2
Percent Yield
 My theoretical yield is 500g but actual
recovery was only 327g
 65.4% recovery
 If the recipe is written to yield 24
muffins, but you only got 21 out of
them,
 87.5% recovery
Molarity!!!!!!!!!!!!!!!!!!!!!!!!
 What is the formula for molarity?
 Molarity = moles solute/L of solution
 How do you find moles if you are given
mass?
 Moles = mass / molar mass (periodic chart)
 What is the formula for a dilution?
 M1V1 = M2V2
Calculate it
 You have 4.5L of a solution that you
added 3.15 moles of NaCl to.
 0.7M
 How many moles of CuBr do you
need to make 10.0L of a 3M solution?
 30 moles
 What is the volume of a 6.3M solution
made from 3.22moles of AgNO3
 0.511 L or 511 mL
What are these?
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
Isotopes?
Atomic Number?
Ions?
Trend in electronegativity?
Trend in ionization energy?
Trend in atomic mass?
Random
 Formula for density?
 D = m/V
 Kelvin conversion?
 K = C + 273
 Ideal Gas Law?
 PV = nRT
 Specific Heat?
 cp= q / m x T
 pH
 -log10[H3O+]
What is . . .
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Standard temperature and pressure?
Oxidation?
Reduction?
Arrhenius Acid/Base?
Bronsted-Lowry Acid/Base?
Who is?
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Thomsson?
Rutherford?
Bohr?
Mendeleev?
Moseley?
What type of reaction is this?
 Na + Cl = NaCl
 Synthesis
 H2 O = H 2 + O 2
 Decomposition
 CxHyOz + O2 = H2O + CO2
 Combustion
 A + BX = AX + B
 Single Replacement
 AX + BY = AY + BX
 Double Replacement
What are these rules?
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Aufbau
Hund’s Rule
Heisenberg Uncertainty Principle
Periodic Law
Pauli’s Exclusion Principle
Which forces hold these atoms and
molecules together?
 H2O
 Intramolecular: Covalent Bond
 Intermolecular: Hydrogen Bonding
 NaCl
 Intramolecular: Ionic
 Intermolecular: Ionic
 NH3
 Intramolecular: Covalent
 Intermolecular: Dipole-dipole
Organic Compounds
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
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Men
MethEat
EthPopcorn & PropButter
But-
 Single is
 Double is
 Triple is
–ane
–ene
-yne
SOL Review
Speed Round
Read each question carefully and choose the best
answer.
1. The average kinetic energy of a sample of water
molecules is
A. Increased as the temperature is increased
B. Increased as the temperature is decreased
C. Unaffected by temperature changes
D. Always equal to zero
2. The element chlorine exists as two naturally
occurring isotopes. Cl-35 occurs 75% of the time
and Cl-37 occurs 25% of the time. Which of the
following calculations should be used to calculate
the correct average atomic mass of chlorine?
A. (35 amu x .75) + (37 amu x .25)
B.
(35 amu x 3) + 37 amu
2
C. (35 amu x 3) + 37 amu
3
D. 35 amu + 37 amu
2
3. The mass of an object was recorded as
9.93 g, 9.90 g, and 10.02 g, using an
electronic analytical balance. What is
the average of these three masses
expressed to the correct number of
significant figures?
A. 9.9 g
B. 9.95 g
C. 10.0 g
D. 10.00 g
4. Which of these shows a volume
of 1.25 liters expressed in
milliliters?
A. 125 mL
B. 12.5 x 101 mL
C. 1.25 x 102 mL
D. 1.25 x 103 mL
5. How does the radioactive isotope C-14 differ from its
stable counterpart C-12?
A. It has a different number of protons and two less neutrons
than C-12
B. It has the same number of protons and two more
electrons than C-12
C. It has the same number of protons but two more neutrons
than C-12
D. It has a different number of protons and two more
neutrons than C-12
6. What is the first step that should be taken when a
caustic chemical gets into a person’s eyes?
A. Identify the chemical
B. Call for an ambulance
C. Flush the affected area with water
D. Apply a neutralizing agent
7. Which of these conclusions can be drawn from
Rutherford’s experiment?
A. Each atom contains electrons.
B. The nucleus of an atom can be split.
C. Each atom contains protons.
D. Atoms are mostly empty space.
8.
Group
Mass Data for
Sample X (g)
Displacement
Data for Sample
X (mL)
1
2.7
3.4
2
1.20
1.5
3
6.2
7.40
According to the above data, which of the following
represents the average density for sample X using
the correct number of significant figures?
A. 1 g/mL
B. 0.8 g/mL
C. 0.81 g/mL
D. 0.821 g/mL
1. Which is the correct formula for iron (III) sulfate?
A. Fe3(SO4)2
B. FeSO4
C. Fe2(SO4)3
D. Fe2(SO3)3
2. Which of these represents the
empirical formula and the
molecular formula, respectively,
for a given organic compound?
a)
b)
c)
d)
CH and C2H2
CH and CH4
CH2 and C2H2
CH3 and C3H12
3. Which of these describes a tendency for atomic
radii as displayed on the periodic chart?
A. Atomic radii decrease left to right across a period.
B. Atomic radii increase left to right across a period.
C. Atomic radii decrease top to bottom down a group.
D. Atomic radii increase, then decrease from top to
bottom down a group.
4. Chlorine forms a 1- ion. How many electrons does
a chloride ion have?
A. 1
B. 16
C. 17
D. 18
?
5. Which of the groups below has the electron dot
structure shown above?
A. Noble gases
B. Halogens
C. Alkali metals
D. Transition elements
6. An element has an electron configuration of
1s22s22p63s2. Which of these will be in the
same group as this element?
A. 1s22s22p6
B. 1s22s22p63s23p64s2
C. 1s22s22p63s1
D. 1s22s22p63s23p6
7. Which of these elements is the
most chemically active?
A. F
B. Cl
C. Br
D. I
1. What is the percentage of aluminum in
aluminum oxide (Al2O3)?
A. 47%
B. 48%
C. 53%
D. 54%
2. A student wanted to calculate the formula for
hydrated copper sulfate. After careful massing,
she heated the compound to remove the water.
She calculated the formula to be CuSO4 . 4H2O.
The actual formula was CuSO4 . 5H2O. What is the
most likely source of analytical error in the
student’s experiment?
A. The water was not completely evaporated from the
compound.
B. The actual mass of the anhydrous CuSO4 was less than
the measurement.
C. The CuSO4 reacted with elemental copper.
D. The atmospheric pressure prevented complete
reaction.
5. Which is an example of a synthesis reaction?
A. HCl + KOH  KCl + H2O
B. Pb(NO3)2 + 2HBr  PbBr2 + 2HNO3
C. Mg + H2SO4  MgSO4 + H2
D. C + O2  CO2
3MgO + 2Al  ?
6. What would be the product(s) of this reaction?
A. 2Mg3Al2O3
B. Mg3Al2 + 3O2
C. 6Mg + Al3O2
D. 3Mg + Al2O3
7. Using the chart above, which of these
combinations will probably form a precipitate?
A. Ammonium chloride
B. Barium bromide
C. Calcium chromate
D. Copper (II) carbonate
8.
Very Active Metal + Water  Metal hydroxide + ?
Which of these completes this reaction?
A. Oxygen
B. Hydrogen
C. Metal oxide
D. Air
9. A compound is composed of 58.8% C, 9.8% H,
and 31.4% O, and the molar mass is 102 g/mol.
What is the molecular formula for this
compound?
A. C2H10O3
B. C5H5O3
C. C5H10O2
D. CH3O3
10.
NaHCO3(s) + HCl(aq)  NaCl(aq) + CO2(g) + H2O(g)
Data Table
Evaporating dish + watch glass
42.70 g
Evaporating dish + watch glass
+ NaHCO3
45.20 g
Evaporating dish + watch glass
+ NaCl
44.45 g
A student conducted an experiment and was interested
in the mass of the product of the chemical reaction.
Some results of the experiment are shown above. What
is the mass of the NaCl?
A. 0.75 g
B. 1.75 g
C. 2.25 g
D. 2.50 g
11. A compound is 50% sulfur and 50% oxygen.
What is the empirical formula?
A. SO4
B. S2O4
C. SO3
D. SO2
A(s) + B(s)  D(g) + heat
12. The reaction shown above is –
A. An endothermic reaction
B. An exothermic reaction
C. A decomposition reaction
D. A double-replacement reaction
13. Which compound contains both ionic and
covalent bonds?
A. NH4Cl
B. MgBr2
C. CH4
D. NH3
1. One of the main assumptions of the
kinetic molecular theory of gases is that
the particles of an ideal gas—
A. must be single atoms instead of molecules
B. are in constant motion
C. must be maintained at very high pressures
D. must be highly chemically reactive
2.
A sample of oxygen gas is collected
over water at 220C and 98.67 kPa
pressure. If the partial pressure of the
water is 2.67 kPa, the partial pressure
of the oxygen is –
A. 93.3 kPa
B. 96.00 kPa
C. 98.66 kPa
D. 101.33 kPa
3.
If the pressure exerted on a
confined gas is doubled, then
the volume of the gas --
A. increases four times
B. decreases by one-fourth
C. is doubled
D. is halved
4. Water can be made to boil above its normal
boiling point of 100oC by –
a. decreasing the air pressure
b. increasing the air pressure
c. increasing the heat being applied
d. decreasing the volume of the
container
Temperature
(oC)
50
25
0
-25
5
10
15
20
Time
(min)
25
5. An experiment yielded the above temperature and time
information. What is the freezing point of the material in
this experiment if the material is a solid at time zero?
a. –25oC
b.
0oC
c. 25oC
d. 50oC
2H2S (g) + 3O2 (g)  2H2O (g) + 2SO2 (g)
6. If 3.50 g of H2S are used in the above
reaction, what will be the theoretical yield
of water in grams?
A. 0.102 g
B. 0.185 g
C. 1.85 g
D. 185 g
CH4 + 2O2  CO2 +2H2O
7. The number of grams of oxygen required for the
complete combustion of 4.00 grams of methane
(CH4) is—
A. 4.00 g
B. 8.00 g
C. 16.0 g
D. 32.0 g
Read each question carefully and
choose the best answer.
1. A solution contains 225 g of glucose, C6H12O6,
dissolved in enough water to make 0.825 L of
solution. What is the molarity of the solution?
A. 0.66 M
B. 0.97 M
C. 1.03 M
D. 1.52 M
2. Which volume will be occupied by a gas
containing 6.02 x 1023 atoms at STP?
A. 1.0 L
B. 11.2 L
C. 22.4 L
D. 44.8 L
3. How many milliliters of 2.00 M H2SO4 are
needed to provide 0.250 mole of H2SO4?
A. 125 mL
B. 1.25 x 101 mL
C. 8.00 x 103 mL
D. 8.00 mL
4. A catalyst accelerates a chemical reaction because
the –
a. catalyst decreases the number of collisions in a
reaction
b. activation energy of the reaction is lowered in the
presence of a catalyst
c. catalyst decreases the concentration of the
reactants
d. temperature of the reaction increases due to the
catalyst
5. In the reaction 2SO2 (g) + O2 (g)  2SO3 (g), which
change would cause the greatest increase in the
concentration of SO3?
a. Decrease the concentration of SO2
b. Decrease the concentration of O2
c. Increase the concentration of SO2
d. Increase the concentration of O2
6. The hydrogen ion concentration is 1 x 10-7. What is
the pH of this solution?
a. 1
b. 7
c. 10
d. 14
7. Each beaker shown above contains 2.2 grams of
iron and 1 liter of 3M H2SO4. Which reaction will
go to completion first and why?
a. Beaker A because of increased surface area.
b. Beaker B because of increased surface area.
c. Beaker A because of a higher concentration level.
d. Beaker B because of a higher concentration level.
8. Four aqueous solutions and their concentrations
are shown in the above illustration. Which of the
solutions is most likely to be the strongest
conductor of electricity?
a. I
b. II
c. III
d. IV
9. If the temperature of a reaction is increased, the
reaction proceeds at a much quicker rate because
the –
a. Activation energy increases
b. Energy of the products increases
c. Frequency of collisions between reactants
increases
d. Energy of the activated complex increases
10. The formula H2SO4 is representative of which
of the following?
a. A catalyst
b. A base
c. An acid
d. An organic compound
11. To remove the sand first and then the salt from a
mixture of sand and salt water, one combination of
techniques you could use would be to first—
A. evaporate and then distill
B. evaporate and then condense
C. filter and then evaporate
D. filter and then condense
12. A student must make a 3M acid solution using a
5M acid solution. Which of these is the safest
way to make the solution?
a. Slowly pour the 5M acid into water.
b. Slowly add water to the 5M acid solution.
c. Mix half the acid with water; then add the
remaining water.
d. Mix half the water with acid, then add the
remaining acid.
First 6 Weeks SOL Answers
1.
2.
3.
4.
5.
6.
7.
8.
A
A
B
D
C
C
D
C
Second 6 Weeks SOL Answers
1.
2.
3.
4.
5.
6.
7.
C
A
A
D
B
B
A
Third 6 Weeks SOL Answers
1.
2.
3.
4.
5.
6.
7.
8.
C
A
B
C
D
D
D
B
9.
C
10.
B
11.
D
12.
B
13.
A
Fourth 6 Weeks SOL Answers
1. B
2. B
3. D
4. B
5. B
6. C
7. C
Fifth 6 Weeks SOL Answers
1. D
6. B
11. C
2. C
7. B
12. A
3. A
8. B
4. B
9. C
5. D
10. C