Transcript CST RTQ Chemistry DRB

“CST RTQ” = “California Standards Test Released Test Questions”
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Init 4/12/2011 by Daniel R. Barnes
Throughout this presentation,
click this button here if you
ever want to skip to the next
slide without any fancy stuff
In other words,
when T goes up,
P goes up.
P1V1
T1
=
P2V2
T2
P1
=
P2
T1
T2
Gay-Lussac’s Law: When all other factors are held constant, the
pressure of a gas is proportional to its absolute temperature.
c =?
b=2
a=2
a2 + b2 = c2
c2 = 8
22 + 22 = c2
c= √8
4 + 4 = c2
c= √4•2
8 = c2
c= √4•√2
c= 2√2
?
?
Science should
not be a popularity
contest.
y = mx + beef
Nor should it be
a matter of
dogmatic
oppression.
e = mchammer
Galileo
Galilei
This model of the atom
has been tested by many
experiments.
(It’s no longer just a little
baby hypothesis.)
P1V1
T1
=
PV = nRT
P2V2
T2
Atomic number
got bigger.
Average
atomic mass
got smaller!
Number of protons = “atomic number”
Just you wait!
When we finally discover it,
it’ll probably be the heaviest element so far.
?
7A
Chlorine and iodine are
in the same
column = column 7A
“properties” = “characteristics”
Because elements in the
same column tend to
have similar properties,
columns are also known
as “families”.
Column 7A is a wellknown family called
the “halogens”
He
Ionization energy =
The energy required to
remove an electron from
an atom.
Which elements on the graph
hold onto their electrons the
strongest?
Alkali metals
Which element on the periodic
table is the strongest? Helium
Where on the PT is helium
found? Upper right corner
“Losers on
the left”
Who are the X’s, then?
Where are the alkali metals
on the PT? Extreme left
So the alkali family must be . . .
The weakest family
X
Where on the periodic table are the
biggest atoms? The lower left corner
Incidentally, how strong are the atoms in the lower left
corner? They are the weakest elements. They give up their
electrons easily.
Where are the smallest atoms on the PT, and how strong are
they? The smallest atoms on the PT are in the upper right
corner. They pull on electrons the strongest.
X
X
How many valence electrons
does silicon have?
2
Argon?
The Lewis
structure for
sulfur . . .
S
Magnesium?
Most of the alpha particles . . .
. . . shot right through.
But the few that hit the nucleus . . .
. . . bounced back, as though
they’d hit something heavy.
Yeah. That’s still too big.
If an atom is this big, then
the nucleus is . . .
. . . much smaller than this
purple dot.
Fundamental
Forces:
(too weak to matter in something gravitational
as small as an atom)
magnetic ?
Gets gradually stronger as electrostatic
protons get closer
“weak” ?“nuclear”
Has zero strength until protons get VERY
close and then suddenly becomes
“strong” forces
overwhelmingly strong.
+ hates +
20
a. The nucleus of an atom is made of protons and neutrons.
b. The protons in an atomic nucleus are positively-charged and
are very close together, so the repulsive force between them is
enormously strong.
c. Because the protons and neutrons in a nucleus are made of
matter, there is an attractive force of gravity between them, but
it is insignificant compared to the much more powerful
electromagnetic and nuclear forces between them.
d. The strong force has zero strength until two particles get very,
very close, and then the strength of the force suddenly
increases to overwhelming power, as though a switch were
suddenly turned on.
+ hates +
Which force?
Which force?
the “STRONG” force
the electrostatic force
mass # = protons
“mass number”
Types of Nuclear
+ neutrons
Radiation
?
“atomic number” = # of protons
Greek
Name
letter
?
a
alpha
particle
?
b
beta
particle
?
g
gamma
particle
Symbol
Effect on
nucleus
mass # -4
!
atomic # -2
mass # no D
atomic # +1
g
mass # no D
atomic # no D
Types of Nuclear Radiation
Mass
Penetration
power
a
alpha
particle
4 amu
low
b
beta
particle
1/1836
amu
medium
g
gamma
particle
0 amu
high
Greek
Name
letter
The lower the
mass . . .
. . . the higher
the penetration.
Nuclear
Chemistry
Post-Quiz
Symbol
g
Noble
gases
Full valence shells
No need to bond
Diatomic
elements:
H2 N2 O2 F2
(gases)
Cl2
Br2
I2
At2 (?)
X X X
X
X
X
+
+
+
+
+
+
+
+
+
+
+
Cations are . . . positive.
++ +
+
+
+
+
+
+
+
The cubic shape of
this object is a clue
+ +
that it is a .salt
. . crystal.
+
+ +
Salt is an ionic
+
compound composed
+ +
of metal cations and
+
+ +
nonmetal anions.
Anions are . . . negative.
- - - -
nonmetal
nonmetal
H makes 1 bond
O makes 2 bonds
N makes 3 bonds
C makes 4 bonds
Element
types
Bond
type
metal &
metal
metallic
metal &
nonmetal
ionic
nonmetal &
covalent
nonmetal
Nitrogen is a nonmetal
Hydrogen is a nonmetal
Carbon is a nonmetal
Oxygen is a nonmetal
There’s one word in the question that pretty much implies covalent
bonds all by itself . . .
All the elements in these molecules are nonmetals.
When a nonmetal bonds with another nonmetal,
the bond will be . . . covalent.
All the elements in these
molecules are nonmetals.
Anions are . . . negative.
-
Cations are . . .
positive. +
+
+
+
+
+
+
+
- -
- - -
-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Plus and minus sittin’ in a tree . . .
B O N D I N G
2+
Ca
F
Neutral = No charge.
No charges  No intermolecular forces.
No imf’s  Molecules fly apart easily
“hydrogen
bond”
H H
H H
+
+
H
H
O
-
The bond in a hydrogen
gas molecule is
nonpolar covalent.
A hydrogen bond is an This means the two atoms
share electrons equally,
example of an
“intermolecular force”. which means the two atoms
remain neutral.
4A
Silicon and germanium
are in the same column
on the periodic table.
Silicon and germanium
are both in column 4A
Silicon and germanium
both have
four valence electrons.
Si
Ge
A bunch of monomer molecules linked
together in a row form a chain-like
molecule called a “polymer”.
Monomer
Polymer
monomer
amino acids
proteins
(20 main kinds)
(including enzymes)
complex carbohydrates
simple monomer
carbohydrates monomer
monomer
(sugars like glucose)
monomer
nucleotides
monomer (A, T [or U], G, C)
monomer
A—T—C—G—G—A—T—C
T—A—G—C—C—T—A—G
(starch, cellulose)
monomer
nucleic acids
(DNA, mRNA,
tRNA)
monomer
How many molecules do you see?
+
+
+
-
-
-
+
+
+
-
-
-
+
+
+
-
HYDROGEN BONDS!
(They’re not covalent!)
33
a. A polymer is a long molecule made of repeating subunits called
“monomers”.
b. Complex carbohydrates include cellulose and starches.
c. Nucleic acids are polymers made of nucleotides.
d. When an amylase enzyme breaks down a starch molecule,
the starch turns into glucose, a simple carbohydrate.
e. The two strands of a DNA double helix stick to each other
because of hydrogen bonds, a kind of intermolecular force.
f. There are 20 different amino acids that can be linked together
in a chain to make proteins.
g. If a protein is made of the right sequence of amino acids, it
might be a catalyst called an “enzyme”.
Such “repeating subunits”
are called “monomers”.
CH2CH(Cl)CH2CH(Cl)CH2CH(Cl)CH2CH(Cl)CH2CH(Cl)
C
Carbon is in group 4A 
A carbon atom has 4 valence electrons 
Carbon needs 4 more valence
electrons to have an “octet” of 8 
1
bond
?
2 bonds
3 bonds
A carbon atom likes to make 4
covalent bonds.
“carbon backbone”
N
N
35
a. Because carbon is in group 4A on the periodic table, it is safe
to assume that a carbon atom has four valence electrons.
b. A nonmetal atom will attempt to form covalent bonds until the
number of electrons in its outer shell equals eight.
c. An “organic” molecule contains at least one carbon atom, often
many of them, linked together in a row to form a “backbone”.
“chain”
d. The number of possible organic chemicals is so huge because
a carbon atom can make four covalent bonds.
amino
acid
amino
acid
amino
acid
amino
acid
amino
acid
Protein is a polymer made of amino acid monomers.
amino
amino
acid
amino
amino
acid
acid
acid
amino
amino
acid
amino
acid
Organic
acid
Chemistry
Post-Quiz
P1
T1
=
P2
T2
Gay-Lussac’s Law: When all other factors are
held constant, the pressure of a gas is
proportional to its absolute temperature.
Q: Why did the
molecules change
direction so often?
A: They kept
colliding with other
gas molecules.
Q: Why is answer “C”
incorrect?
A: Molecules in the air
travel at about 1000
mi/h. That’s FAST.
NOTE: due to animation limitations, I couldn’t make the particles
change speed every time they changed direction. I apologize.
An “mL” is a unit of volume.
In this story, the volume of the gas . . .
went down.
According to Boyle’s Law, when the
volume of a gas goes down, the
pressure of the gas goes up.
An “mm Hg” is a unit of pressure.
Even without doing any math, which answers can you
eliminate and why?
Answers “A” & “B” must be wrong because
the pressure has to go up.
Why is answer “C” better than answer “D”?
If V is divided by 2, then P must be multiplied by 2.
?
?
According to Charles’ law, heating a gas makes
its volume go up. In other words, it makes the gas expand.
So how could a gas “decrease in volume” (shrink) when
heated? Shouldn’t just the opposite happen?
Well, according to Boyle’s law, you can make a gas shrink by
increasing the pressure on it.
Without even doing any math, you
should be able to predict that if the
temperature is doubled and everything
else remains constant, then the volume
must also double.
20 L x 2 = 40 L
Keep in mind that all gases pretty much
behave the same, so you can safely
ignore the identity of the gases here.
This question is
mostly a matter of
pure memorization.
What would this
number have had to
be in order for “B” to
be correct?
What’s the matter with “0 K”?
Zero kelvins is not equal to zero degrees Celsius.
Zero kelvins is equal to -273 degrees Celsius.
oC + 273
0 = -273
You should recognize
answer “D” as standard
temperature and pressure,
also known as “STP”.
Observant students might
notice that 11.2 liters is
exactly half of 22.4 liters.
At STP, two moles of gas should occupy 44.8 L.
At STP, 0.1 moles of gas should occupy 2.24 L.
At STP, ten moles of gas should occupy 224 L.
At STP, 100 moles of gas should occupy 2240 L.
423
-273
150
To turn degrees Celsius into kelvins, you add 273.
To turn kelvins into degrees Celsius, you subtract 273.
What is a “vacuum”?
A vacuum has no matter in it, not even
any gas. A vacuum is airless and empty.
No gas molecules means no gas
pressure.
Gas pressure is caused by gas molecules
colliding with each other and with the
walls of their container.
A pressure of zero occurs at 0 K because at this temperature,
known as “absolute zero”, molecules stop moving.
If molecules are not moving, they can’t collide with anything.
No collisions, no pressure.
= 273 K ≠ 0 K
The temperature at which molecular motion stops is known
as “absolute zero”.
It turns out that zero kelvins (0 K) is equal to -273 oC. Since
molecules can’t go any slower than a complete stop, -273 oC
is the coldest possible temperature.
Based on -273 oC being the coldest possible temperature,
which answer must be incorrect?
“B” can’t be correct because there’s no such thing as a
negative kelvin temperature. Zero is as low as kelvins goes.
Water and ethanol are both liquids.
If you mix them and there is less ethanol
than water, ethanol is the solute.
A solute dissolves
If there is more ethanol than water,
in a solvent to form
ethanol is the solvent.
a solution.
In salt water, the
salt is the solute
because it turns
from a solid to a
liquid as it
dissolves.
In general, whoever changes his state of
matter (“phase”) during mixing is the solute.
If both substances are the same state of
matter before and after mixing, the solvent
is the substance that there is more of.
A solution is made of a solute
dissolved in a solvent.
In this example, the coffee crystals
are the solute because they change
from solid to liquid.
Water is known as the “universal solvent” because
so many things dissolve in water, and when they do,
the water remains liquid.
If water was famous for changing into a solid or a gas
when it mixed with things, it might be known as the
“universal solute” instead.
+
+
H
+
H
-
O
+
-
+
+
+
H
H
H
O
-
+
H
H
-
O
+
O
-
H
+
H
H
O
O
H
H
+
+
-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Cl-
Na+
Cl-
Na+
Cl-
Na+
Cl-
Na+
In this example,
the salt is the
solute, the
water is the
solvent, and the
salt water is the
solution.
You are now ready to eliminate two answer choices . . .
So who is the
“nonpolar solute”?
Oil and water don’t
mix.
Nonpolar and polar
don’t mix.
Your chance of success just
increased from 25% to 50%!
gas
exothermic
liquid
solid
endothermic
At that point,
the solution was
“saturated”.
Heat is a very disorderly form of energy, so if you’re going up
the ladder, heat is your friend. If you’re going down the
ladder, heat is your enemy. [C & C: salt water vs. soda.]
There is a limit to everything.
You can only dissolve so much NaCl
(salt) in H2O (water).
“Solubility” is how easy it is to dissolve a
solute in a solvent.
The bigger the number, the more soluble
the solute is.
In this problem, solubility is expressed in grams of solute per
100 grams of solvent.
The more solvent you have, the more solute you can dissolve
in it before the solution becomes saturated. When a solution
is saturated, no more solute can dissolve in it.
It stands to reason that if you have half as much solvent, you
can only dissolve half as much solute. “18.1 g” is correct
because 18.1 is one half of 36.2.
THE BIG PICTURE:
HNO3 is being dissolved in water to make an
aqueous solution of HNO3.
M = mol/L = a way of expressing concentration
concentration =
solute
solution
solute = ? mol
solution = 5 L
concentration = 2 M = 2 mol/L
solution x concentration =
solute
solution
x solution
solution x concentration = solute
solute = solution x concentration = 5 L x 2 mol/L
solute = 10 mol
concentration =
solute
solution
332 g
1,000,000 ppm
c=
x
1000 g
1
c = 332 x 1000 ppm = 332,000 ppm
It make sense that the grams are
canceling each other out because
we don’t want grams in our
answer.
The only unit we want in our
answer is ppm.
gas
liquid
solid
In a solid, particles are stuck in place,
Right now, the but they do jiggle and vibrate.
motion of the In a liquid, particles are free to wander,
particles is
but they must stay huddled together.
pretty . . .
In a gas, particles are free to fly all over
the place.
exothermic
liquid
solid
endothermic
gas
PHOTOSYNTHESIS:
water + carbon dioxide + sunlight  sugar + oxygen
6H2O + 6CO2 + energy  C6H12O6 + 6O2
In the chemical equation for photosynthesis, energy is on the
left side of the arrow, so the reaction is endothermic.
COMBUSTION:
CnH2n+2 + O2  CO2 + H2O + energy
-196 oC
K = oC + 273
oC = K - 273
oC = 77 – 273 = -196
Cp = 0.4 J/goC
Ti = 20 oC
Q=?J
m = 30 g
Tf = 60 oC
Q = m DT Cp
DT = Tf - Ti = 60 oC – 20 oC = 40 oC
Q = (30 g)(40 oC)(0.4 J/goC)
Q = (1200)(0.4 J) = 480 J
acid
base
Watch how the OH- from the base
grabs onto (“accepts”)
the H+
Acids give NaCl Bases give
the acid.
HCl + NaOH  NaCl +from
H2O
off
H+ ions
off OH- ions
is a NEUTRALIZATION reaction.
+Cl+OHH
HCl
Na
NaOH
H+ ions
OH- ions
make acids
taste sour
HOH
H2O
make bases
taste bitter.
NEUTRAL
NaCl(aq)
His
hindquarters
turned into
SOAP!
60
a. What ion do acids give off?
b. What ion do bases give off?
“hydrogen ion” = H+
“hydroxide ion” = OH-
c. What do you call the reaction between an acid and a base?
neutralization
d. What two things are formed during a neutralization reaction?
water and some kind of salt
e. What kinds of solutions feel slippery between your fingers?
bases (a.k.a. “alkaline” solutions)
f. What do bases turn your flesh into?
soap
g. What pH is considered to be “neutral”?
7
h. What pH is considered to be “acid”?
<7
i. What pH is considered to be “basic”?
>7
Answers “A”, “B”, and “D”
are all electrolytes.
+++
NH
Na
C12H
H224O11
SO
NO
Cl4-32--
All three of these substances
break up into ions when
dissolved in water.
NO IONS,
NO CURRENT,
NO LIGHT!
Ions that are free to wander
can carry electric current,
so electrolytes are good
conductors when they are
dissolved in water.
HCl  H+ + ClNaNO  Na+ + NO -
3
3
Sugar
dissolves in (NH ) SO  2NH + + SO 24 2
4
4
4
water, but it
doesn’t break
H2O
up into ions. C12H22O11(cr)  C12H22O11(aq)
61
a. What do you call a material that breaks up into ions in water?
an “electrolyte”
b. Because they break up into ions in water, electrolytes make
good conductors when aqueous.
c. Why does salt water conduct electricity but sugar water
doesn’t?
Salt breaks up into ions in water, but sugar molecules don’t.
Aqueous
HCl(aq)
solution of
hydrochloric
acid
?
?
?
GET
NEUTRALIZED
Tiny bubbles of
flammable
hydrogen gas.
Shiny chunks of zinc metal
62
a. What happens when an acid and a metal react?
As the metal dissolves to become a salt,
bubbles of flammable hydrogen gas are created.
b. What kinds of solutions feel slippery to your fingertips and why?
Bases because they turn you into soap.
c. An acid will turn into a salt if you mix it with either a metal or a
base, but not if you mix it with another acid.
d. What do you call the reaction that happens when you mix an
acid with a base?
neutralization
Cu(NO3)2 + 2H2O  Cu(OH)2 + 2HNO3
Cu(OH)2 is a metal hydroxide.
Therefore, Cu(OH)2 is a base.
Mr. Barnes,
Acids and bases neutralize
each other
can I take a
to form salt and water. nap? My
brain wants to
exploding.
Because copper
(II) nitrate is
soluble and
copper
hydroxide isn’t,
turning copper
hydroxide into
copper nitrate
decreases the
amount of solid
in the test tube.
The brightness of the
bulb shows us that KOH
is a strong electrolyte.
All strong acids and
strong bases are also
strong electrolytes.
?
?
?
OH- = the hydroxide ion. Get to know it!
H2O
K+
OHWhen you put potassium hydroxide crystals in water, the
KOH dissolves into positive potassium ions and negative
hydroxide ions.
Anything that gives off OH- ions in water is a base.
KOH(cr)  K+(aq) + OH-(aq)
A base that COMPLETELY ionizes in water is a “strong” base.
?
?
?
?
What kind
material
pH of 11? Acids &
Theofhigher
thehas
pH, athe
Bases Postmore
basic
the
material
is.
What kind of material has a pH of 7?
Quiz
What kind of material has a pH of 5?
What does
Pure water is
What kindconsidered
of materialto
has a pH of 3? “alkaline”
mean?
be “neutral”.
N
ACID
BASIC
E
U
T
R
A
L
So which is MORE acidic?
The lower the pH, the
ph = 5 or pH = 3?
more acid the material is.
REACTANTS
 PRODUCTS
The chemicals on the left side of the arrow are called . . .
The chemicals that the reactants turn into are called . . .
?
?
?
As time goes by during a chemical reaction,
the amount of reactants decreases and
the amount of products increases.
REACTANTS
?
?
?

PRODUCTS
Increasing the
concentration
of a product
doesn’t speed
up a reaction.
In fact, if the
reaction is
reversible, it
may make the
reaction go in
reverse!
Reactions
go fasterof
when
the chemicals
are
Increasing generally
the concentration
a reactant
will make
a hotter.
Why
you
suppose
this
ismolecules
true? the concentration
reaction
go faster.
Decreasing
ofthey
a
Whendo
chemicals
are hotter,
move faster, so
reactant
will make
a reaction
gooften.
slower.
hit
each other
harder
and more
Heat speeds up
reactions.
?
If you want to
slow down a
reaction,
remove
reactants, not
products.
?
?
Adding reactants speeds up a reaction.
In a chemical reaction, atoms are not created or destroyed,
and they don’t change element, but they do change
who they’re stuck to.
In a chemical reaction, old bonds must break in order for
new bonds to form.
Breaking bonds means ripping things apart that are attracted
to each other. That’s hard work. It costs energy.
The amount of energy required to break old bonds during a
reaction is called “activation energy”.
If you provide reactants with enough activation energy (Ea),
they will form an activated complex and may then turn into
products.
A catalyst facilitates a reaction by lowering the amount of
activation energy required to form the activated complex.
A catalyst “digs a tunnel through the activation energy hill”.
Pt
It takes energy to
2CO + O2  2CO2 + energy
break old bonds,
but takes less energy
when a catalyst is helping.
Ea
*
C O
O O
C O
This is just a definition question. Do
you know the definition of a catalyst?
Then you got this question right.
Answer “C”, an inhibitor, is a material
that interferes with a catalyst. An
inhibitor is a sort of anti-catalyst.
You could somewhat be forgiven for picking “D”, a reactant,
because adding more reactant does speed up a reaction.
However, reactants don’t lower activation energy.
3
2
2
N= 1 2
H= 3 6
O= 2 3
3
N= 2
H= 2 6
O= 1 3
Now, the equation is
balanced, and the
coefficient in front of the
NH3 is . . . 2
However, “2” is answer A, and the answer key says the correct
answer is C.
4 2
3
3 2
N= 1 2
H= 3 6
O= 2 3
21
63
N= 2
H= 2 6
O= 1 3
Perhaps the chemistry wizards in the
California department of education don’t like
using fractions as coefficients.
In this particular equation, it’s okay to use an
odd number over two as a coefficient for O2
because O2 is a diatomic element.
However, if you really hate using fractions as coefficients, there is
a solution: multiply every coeffcient by two.
4 2
3
3 2
N= 1 2 4
H = 3 6 12
O= 2 3 6
21
63
N= 2 4
H = 2 6 12
O= 1 3 6
Of course, if you double all the coefficients,
you also have to double the atom counts.
The equation is still balanced, and now, the
coefficient in front of NH3 is a “4”.
This is not a good question.
You should never write multiple choice question for which there is
more than one correct answer. Maybe that’s why the CA DoE
ACIDS & BASES STANDARDS
Please copy the following onto your note paper.
They are the SWBAT’s for this lesson.
Click this button
when you’re ready
to continue.
Acids & Bases Post-Quiz
Answer the following using complete sentences on a piece of
notebook paper:
1. What ion do acids give off? What ion do bases give off?
2. What do you call the reaction that happens when an acid and a
base get together? What is formed by this kind of reaction?
3. What pH do acids, bases, pure water, and salt water have?
4. What kind of solution feels slippery and why?
5. What happens when acids and metals get together?
6. What is the difference between a weak acid and a strong acid?
What do strong acids and strong bases have in common?
When you’re done, discuss your answers with your partner.
Anyone who is called on will be representing both himself
and his partner when he gives his answer to the class.
Acids & Bases Further Development
BARNES!
Make some
application/synthesis/analysis/evaluation questions
to really put the ideas to work rather than simply
demanding myna bird-style regurgitation.
O-CHEM STANDARDS
Please copy the following onto your note paper.
They are the SWBAT’s for this lesson.
Click this button
when you’re ready
to continue.
Organic Chemistry Post-Quiz
Answer the following using complete sentences on a piece of
notebook paper:
1. What is a polymer?
2. What element is at the heart of organic chemistry? Why?
3. What monomers are proteins made of?
4. Compare and contrast starch and cellulose.
5. What are A, C, T, and G?
6. What is an enzyme? Why does it have the powers that it
does?
When you’re done, discuss your answers with your partner.
Anyone who is called on will be representing both himself
and his partner when he gives his answer to the class.
NUCLEAR STANDARDS
Click this button when you’re ready to continue.
Nuclear Chemistry Post-Quiz
Answer the following using complete sentences on a piece of
notebook paper:
Press me when you’re done discussing questions #’s 1-6
1. Compare and contrast atomic number and mass number.
2. What happens to a nucleus as a result of alpha decay?
3. What are the three main particles given off by radioactive
atoms? Compare their penetration powers and their masses.
4. What happens when a neutron in a nucleus breaks up into a
proton and an electron?
5. What is an atomic nucleus made of? How big is it?
6. What holds a nucleus together? Why is this force so
necessary for a nucleus to stay together as a single particle?
When you’re done, discuss your answers with your partner.
Anyone who is called on will be representing both himself
and his partner when he gives his answer to the class.
Nuclear Chemistry Post-Quiz
WAIT! THERE’S MORE! SURPRISE BONUS QUESTIONS!
BONUS #1: In the formula e = mc2, what do all the symbols stand
for?
BONUS #2: Why are some isotopes of some elements
radioactive, while other isotopes are not radioactive? (Example:
carbon-12 is not radioactive, but carbon-14 is radioactive.)
(These topics are mentioned in the standards, but are not
addressed by the CST RTQ’s, so they need to be addressed
at least once before the CST happens.)
Title page
Investigation &
Experimentation
Questions
(interactive table of contents)
Bonding
Questions
page -1
Heat
Questions
Answer Key
Organic
Chemistry
Questions
Acids, Bases,
& Salt Solutions
Questions
Atomic Structure
Questions
Gas Questions
Reaction Rate &
Equilibrium
Questions
Nuclear
Questions
Solution
Questions
Balancing &
Stoichiometry
Questions
Periodic Table
Questions
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particular
question
number
Title page
(interactive table of contents)
Question #1
Question #31
Question #61
Question #6
Question #36
Question #66
Question #11
Question #41
Question #71
Question #16
Question #46
Question #76
Question #21
Question #51
Question #81
Question #26
Question #56
Question #86
page zero
Answer Key
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