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AP Chemistry Full Year Review

Total questions: 120

Worksheet time: 4hrs 17mins

Name
Class
Date
1.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
2.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
3.
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4 (Lewis structure is shown) .
a)
eg = tetrahedral, mg = tetrahedral
b)
eg = linear, mg = linear
c)
eg = octahedral, mg = square planar
d)
eg = trigonal bipyramidal, mg = tetrahedral
4.
Bond angle for tetrahedral
a)
120o
b)
109.5o
c)
104.5o
d)
107o
5.
Bond angle for bent
a)
120o
b)
109.5o
c)
104.5o
d)
107o
6.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (show your work)

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

7.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
8.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
9.

Steel is an example of a/an _______________ alloy because carbon atoms move between the iron atoms’ crystal structure.

a)

eutetic

b)

interstitial

c)

substitutional

d)

vacancy

10.

Pb + 2Ag+ → Pb+2 + 2Ag


The chemical species being reduced is

a)

Ag

b)

Pb

c)

Pb+2

d)

Ag+

11.
What is oxidation number of Cr in Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
12.
Which change does nitrogen undergo oxidation?
a)
A
b)
B
c)
C
d)
D
13.
What reaction occurs at the anode?
a)
Ag+ + e- →Ag
b)
Ag → Ag+ + e-
c)
Ni2+ + 2e- → Ni
d)
Ni → Ni2+ + 2e-
14.

why would O2 effuse faster than CO2 in the same room

a)

because it has more energy

b)

because it has a smaller molar mass

c)

because oxygen has a higher temperature

d)

they will effuse the same because the temperature is fixed

15.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
16.
Nitrogen has three occurring isotopes: Nitrogen-13, Nitrogen-14, Nitrogen-15. Which isotope is the most abundant?
a)
Nitrogen-13
b)
Nitrogen-14
c)
Nitrogen-15
d)
Based on the information given, it cannot be determined
17.
Acidic buffer is made up of
a)
weak acid and weak base
b)
weak acid and its conjugate salt
c)
weak acid and its conjugate base
d)
strong acid and its conjugate base
18.
Which solution A and B of equal volume and concentration mixed together to form a buffer?
a)
Nitric acid and potassium hydroxide
b)
Nitric acid and potassium nitrate
c)
Propanoic acid and potassium hydroxide
d)
Propanoic acid and potassium propanoate
19.
What is the pH of a 0.08 M solution of HNO3?
a)
1.10
b)
0.832
c)
12.9
d)
13.2
20.

Complete the sentence.

A substance that is more acidic has a _____ pH, and ____H+ than a substance that is basic.

a)

lower, more

b)

higher, less

c)

the same

d)

none of the above

21.
The equilibrium constant for reaction 1 is K.  What is the equilibrium constant for equation 2?
(1) SO2(g) + 1/2O2(g) ↔ SO3(g)
(2) 2SO3(g) ↔ 2SO2(g) + O2(g) 
a)
K squared  (K2)
b)
2K
c)
1/2K
d)
1/K squared  (1/K2)
22.
The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H2O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if 15.0mL of acid neutralized?
a)
0.8M
b)
1.2M
c)
12.5M
23.

In which of the following aqueous solutions does the weak acid exhibit the highest percentage of ionization?

(Remember : 1. the stronger the acid, the greater is the percent ionization; 2. diluting the solution increases the percent ionization)

a)

.01 M HC2H3O2 . (Ka 1.8 x 10 -5)

b)

.01 M HNO2 . ( Ka =4.5 x 10 -4)

c)

.01 M HClO . (Ka= 3.0 x 10 -8)

d)

.01 M HF (Ka= 6.8 x 10 -4)

24.
The solubility of Cd(OH)2 in water is 1.67 x 10-5 mol/L. The Ksp value for Cd(OH)2 is
a)
1.86 x 10-14
b)
4.66 x 10-15
c)
5.58 x 10-10
d)
1.67 x 10-5
25.
The correct mathematical expression for finding the molar solubility (s) of Sn(OH)2 is:
a)
2s2 = Ksp
b)
2s3 = Ksp
c)
4s3 = Ksp
d)
8s3 = Ksp
26.
The pH at the equivalence point of the titration of a strong acid with a strong base is usually:
a)
acidic 3.9
b)
acidic 4.5
c)
neutral 7.0
d)
basic 8.2
27.
A student performs an acid-base titration and plots the experimental results in the graph above.  Which of the following statements best explains the experimental findings?
a)
A weak acid was titrated with a strong base, as evidenced by the equivalence point at pH >7.
b)
A weak acid was titrated with a weak base, as evidenced by the equivalence point a pH approximately 7.
28.
HX(aq) + Y-(aq) <--> HY(aq) + X-(aq)          Keq > 1
Based on the information given above, which of the following is the strongest acid?
a)
HX
b)
HY
29.
Based on the Ksp values in the table above, a saturated solution of which of the following compounds has the highest [Cl-]?
a)
PbCl2
b)
CuCl
c)
AgCl
d)
Hg2Cl2
30.

Does a precipitate form when 0.050 L of 2.0x10-2M Pb(NO3)2 is mixed with 0.010 L of 1.0x10-2M Na2SO4? (PbSO4 has a Ksp = 3 x 10-28)

a)

Yes Qsp = 2.84x10-5

b)

No Qsp = 2.84x10-35

c)

Yes Qsp = 3.14x10-5

d)

No Qsp = 3.14x10-35

31.
What is oxidation number of P in K3PO4?
a)
+1
b)
+5
c)
-2
d)
0
32.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
33.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
34.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements. (keep two decimal places throughout calculations)
a)
SO
b)
SO2
c)
SO3
d)
SO4
35.
Find the percent composition of N2S2.
a)
N: 69.6%  S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
36.
How many moles are in 88 g of propane, C3H8. 
a)
2.0
b)
16.0
c)
0.051
d)
3,872
37.
Epinephrine (adrenaline) is a hormone secreted into the bloodstream in times of stress. It contains 59.0%  C, 7.15% H, 26.20%O, 7.65%N and has a molar mass of 183 g/mol. What is its molecular formula? 
a)
C9H13NO3
b)
C5H11N3O2
c)
C8H12NO2
d)
C7H9N2O
38.
1 P4 + 3 O2 --> 1 P4O6 
What is the limiting reactant if 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6 
d)
none of the above
39.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
40.
If the pressure exerted by a gas at 25 degrees C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?
a)
.002766 mole
b)
.0069 mol
c)
2.766 mol
d)
9.887 mol
41.

Yellow dye is separated from a mixture using a polar stationary phase (filter paper) and non-polar mobile phase (solvent). The yellow dye is:

a)

polar

b)

nonpolar

42.

What formula do we use for dilution calculations?

a)

M1V1=M2V2

b)

D=m/V

c)

V1=M2

d)

Total Volume/Partial Volume

43.

Losing electrons is ________________, gaining electrons is ________________

a)

oxidation, reduction

b)

reduction, oxidation

44.

The ______ the acid, the ______ its conjugate base.

a)

stronger, weaker

b)

stronger, stronger

45.

What coefficients balance this equation? ___Na + ___ZnI2 → ____NaI + ___Zn

a)

1,2,1,2

b)

2,1,2,1

c)

2,2,2,1

d)

1,1,2,1

46.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
47.

The conjugate base of H2SO4 is ___.

a)

H2SO3

b)

HSO4-1

c)

H3SO4+1

d)

SO4-2

48.

NH3 + H2O ↔ NH4+ + OH-

What is H2O in this reaction?

a)

acid

b)

base

c)

conjugate acid

d)

conjugate base

49.

What type of bonding is found within a water molecule?

a)

ionic bonding

b)

polar covalent bonding

c)

nonpolar covalent bonding

d)

hydrogen bonding

50.

The Lewis structure of which compound is best represented with resonance structures?

a)

MgCl2

b)

CO2

c)

SO3 2-

d)

OCl2

51.

The molecule shown above represents alanine, one of the simplest amino acids. This amino acid is considered nonessential to the human diet as it can be synthesized in the body from other compounds.

Which statement is correct concerning alanine?

a)

Each carbon atom is sp3 hybridized.

b)

The hybridization of the nitrogen atom is sp2.

c)

All bond angles are approximately 109.50.

d)

The molecule contains 12 sigma and 6 pi bonds.

52.

Which bond is the most polar?

a)

F-O

b)

H-O

c)

Na -O

d)

Sn-O

53.

Which of the following compounds would have the highest lattice energy?

a)

LiF

b)

MgCl2

c)

CaBr2

d)

C2H6

54.

What is the molecular geometry in the structure A?

a)

Tetrahedral

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Octahedral

55.

Which structure is more likely to correspond with the actual Lewis diagram for the sulfate ion?

a)

Structure A; single bonds are more stable than double bonds

b)

Structure A; it has the most unshared pairs of electrons

c)

Structure B; there are more possible resonance structures

d)

Structure B; fewer atoms have formal charges

56.

Which of the following typically has the lowest melting point?

a)

Metals

b)

Covalent network solids

c)

Ionic compounds

d)

Covalent molecules

57.

Which of the following probably has the highest solubility in hexane, C6H14?

a)

Metals

b)

Polar covalent molecules

c)

Ionic compounds

d)

Nonpolar covalent molecules

58.

Of the following molecules, which is the most polar?

a)

CO

b)

CO2

c)

O2

d)

HF

e)

F2

59.

Which of the following has the lowest melting point?

a)

Zn

b)

SiO2

c)

CaCl2

d)

C2H6

60.
Which of these typically increases when intermolecular forces increase?
a)
Boiling Point
b)
Melting Point
c)
Viscosity
d)
All of these
61.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

62.

1. Under which conditions does a real gas behave very much like an ideal gas?

a)

high temperature and low pressure

b)

high temperature and high pressure

c)

low temperature and high pressure

d)

low temperature and low pressure

63.
You have a 0.5 M MgSO4 stock solution available.  Calculate the volume of the stock solution needed to make 2.0 L of 0.20 M MgSO4.
a)
0.8 L
b)
5 L 
c)
0.1 L
d)
0.5 L
64.

What order is this graph?

a)

Zero

b)

First

c)

Second

d)

Third

65.

What order is this graph?

a)

Zero

b)

First

c)

Second

d)

Third

66.

If you quadruple the concentration and the rate quadruples, what order is this reaction?

a)

zero

b)

first

c)

second

67.

Which step of a reaction mechanism determines the rate?

a)

the slow step

b)

the fast step

c)

the first step

d)

the second step

68.

What order is the half life of Carbon14?

a)

Zero

b)

First

c)

Second

69.

What is the unit for the rate constant (k) for 2nd order reactions?

a)

s-1

b)

M/s

c)

M-1s-1

70.

How does a catalyst speed up a reaction?

a)

Adding more reactant

b)

Providing a pathway that has a lower activation energy

c)

Increasing the activation energy

d)

Increasing binding energy

71.

___________ are produced in one step and used up in a later step and __________________ are present and unchanged in the reactants and the products

a)

intermediates, catalysts

b)

catalysts, intermediates

72.

If a “reaction profile” has a taller ‘hill’ (or activation energy) then the reaction is ____________________?

a)

Faster

b)

Slower

73.

What are the 2 characteristics that an effective collision must have? SELECT TWO

a)

Enough energy to overcome Ea

b)

Molecules in the correct orientations

c)

High enough temperature

d)

Apporpriate intermediates present

74.

What is the rate law for the reaction with this slow elementary step? A --> B + C

a)

rate = k[A]2

b)

rate = k[B]2

c)

rate = k[A][B]

d)

rate = k[A]

75.

What is the rate law for the reaction with this slow elementary step? A + 2B --> D + C

a)

rate = k[A]2

b)

rate = k[A][B]2

c)

rate = k[A][B]

d)

rate = k[A]

76.

Which curve represents the most particles in this Maxwell-Boltzmann curve (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

They all have the same number of particles

77.
a)
A. is most exothermic
b)
B. is most exothermic
c)
C. is most exothermic
d)
D. is most exothermic
78.
Consider the following rate law: Rate = k[A]n[B]m
How are the exponents n and m determined?
a)
by using balanced chemical equation
b)
By using the subscripts for the formulas
c)
By educated guess
d)
By experiment 
79.
step 1: O3 → O2 + O
step 2: O3 + O → 2 O2

The oxygen atom (O) is considered to be a(n)...
a)
reactant
b)
catalyst
c)
reaction intermediate
d)
activated complex
80.
A compound has a half-life of 14 min. How much time will it take a 12 mol sample to decay to 1.5 mol?
a)
14 min
b)
28 min
c)
42 min
d)
56 min
81.
a)
IO-, because it was used as a reactant in an earlier step and reproduced in a subsequent step
b)
I-, because it was used as a reactant in an earlier step and reproduced in a subsequent step
c)
IO-, because it was produced in an earlier step and used up in a subsequent step
d)
I-, because it was produced in an earlier step and used up in a subsequent step
82.
Multi-step (Consecutive) Reactions:
Mechanisms in which one elementary step is followed by another are very common.
step 1:              A + B → Q
step 2:              B + Q → C
net reaction:    A + 2B → C
Which of the following is false?
a)
The net reaction is just the sum of its elementary steps.
b)
The species Q is an intermediate, usually an unstable or highly reactive species. 
c)
Intermediates such as Q can appear in the rate law of a net reaction.
d)
If both steps proceed at similar rates, rate law experiments on the net reaction would not reveal that two separate steps are involved here.The rate law for the reaction would berate=k[A][B]2
83.
The rate law for a reaction is rate = k [A][B]2 Which one of the following statements is false? 
a)
A) If [B] is doubled, the reaction rate will increase by a factor of 4. 
b)
B) The reaction is second order in B.
c)
C) The reaction is first order in A.
d)
D) The reaction is second order overall.
84.

The graph shown depicts the relationship between concentration and time. What is the slope of this line?

a)

-k

b)

-1/k

c)

k

d)

ln[A]o

85.

In an exothermic reaction, the sign of ΔH is ____ and the reaction feels ______

a)

(-), hot

b)

(+), hot

c)

(-), cold

d)

(+), cold

86.

Freezing is an _________________________ process

a)

Endothermic

b)

Exothermic

87.

Breaking bonds is _________________. Forming bonds is ______________________

a)

endothermic, exothermic

b)

exothermic, endothermic

88.

ΔHrxn = ΔH_________________ − ΔH_________________

a)

products, reactants

b)

reactants, products

89.

According to Hess' Law, if you double the coefficients of a reaction, ΔH will ________________________

a)

Stay the same

b)

Double

c)

Quadruple

d)

Halve

90.

According to Hess' Law, if you reverse a reaction, ΔH will ________________________

a)

Change signs

b)

Double

c)

Be inversed

d)

Halve

91.

Exothermic

a)

absorb energy

b)

release energy

92.

Endothermic

a)

absorb energy

b)

release energy

93.

In a system, the energy lost by the reacting species must be ________________ the energy gained by the surrouding

a)

greater than

b)

less than

c)

equal to

94.

Using bond energies to solve for enthalpy, 

a)

ΔH\Delta H  =  Bond broken - bonds formed

b)

undefined =  Bond formed- bonds broken

c)

undefined =  products - reactants

d)

undefined =  reactants- products

95.

At equilibrium, rates of the forward and reverse reaction are...

a)

The same

b)

Not the same

96.

At equilibrium, concentrations of reactants and products are

a)

equal

b)

constant

97.

At what time does the system first reach equilibrium?

a)

24s

b)

40s

c)

60s

d)

80s

98.

The equilibrium constant expression, Kc, given aA + bB ⇄ cC + dD, is...

a)

Kc = [C]c[D]d[A]a[B]bK_c\ =\ \frac{\left[C\right]^c\left[D\right]^d}{\left[A\right]^a\left[B\right]^b}  

b)

Kc = [A]a[B]b[C]c[D]dK_c\ =\ \frac{\left[A\right]^a\left[B\right]^b}{\left[C\right]^c\left[D\right]^d}  

99.

Which substance(s) would not be included in a equilibrium constant expression?

a)

NaCl(s)

b)

NaCl(aq)

c)

NaCl(l)

d)

NaCl(g)

100.

If a K value is greater than 1,

a)

more products are present at equilibrium

b)

more reactants are present at equilibrium

101.

If K < Q, the reaction will proceed in the...

a)

reverse direction to reach equilibrium

b)

forward direction to reach equilibrium

102.

To calculate the K of an overall reaction from individual reaction K values, the individual K values are

a)

added

b)

subtracted

c)

multiplied

d)

divided

103.

When the coefficient of a reaction is multiplied by a factor x,

a)

the K value is multipled by x

b)

the K value is divided by x

c)

the K value is raised to the power x

104.

Given the following equilibrium equation,

A (g) + 2B (g) ⇄ AB2 (g) ΔH > 0, which of the following changes will increase the amount of AB2 in the vessel?

a)

Decreasing the temperature

b)

Increasing the concentration of A

c)

Removing a small amount of B

d)

Decreasing the pressure

105.

Given the following equilibrium equation,

A (g) + 2B (g) ⇄ AB2 (g) ΔH < 0, which of the following changes will decrease the amount of AB2 in the vessel?

a)

Increasing the temperature

b)

Increasing the concentration of A

c)

Increasing the pressure

d)

Adding a catalyst

106.

The following system at equilibrium is exothermic. If the temperature is increased...

A (g) + 2B (g) ⇄ AB2 (g)

a)

[A] will increase the most

b)

[B] will increase the most

c)

[AB2] will increase the most

107.

If a common ion is present, the solubility of a salt

a)

is increased

b)

is decreased

c)

will remain the same

108.

If pOH=4.5, pH=?. and is the solution acidic, basic, or neutral

a)

9.5

Basic

b)

11.2

Basic

c)

6.25

Acidic

d)

7

Neutral

109.

If [H] = 1 x10^-7, pH= ?. Is the solution acidic, basic, or neutral

a)

7

Neutral

b)

2.3

Acidic

c)

11.34

Basic

d)

7.5

Basic

110.

What two values are equal to the equivalence point of a titration

a)

Moles of Acid and Moles of Base

b)

Volume of Acid and Volume of Base

c)

Moles and Volume of Acids Only

d)

Moles and Volume of Base Only

111.

A process which causes a decrease in entropy is

a)

condensation of steam to form liquid water

b)

vaporization of liquid water to form steam

c)

dissociation of solid sodium chloride into aqueous sodium cations and chloride anions

d)

sublimation of snow to water vapor

112.

reaction is ALWAYS thermodynamically favorable

a)

- H, - S

b)

+ H, + S

c)

+ H, - S

d)

- H, + S

113.

a reaction that is exothermic and has a decrease in entropy is

a)

spontaneous at high temps

b)

spontaneous at low temps

c)

always spontaneous

d)

never spontaneous

114.

For which of these processes is the value of ΔS\Delta S  expected to be negative?
I. NaCl is dissolved in water.
II. Steam condenses to liquid water.
III.  MgCO3MgCO_3   is decomposed into MgO and  CO2CO_2  .

a)

I only

b)

I and III only

c)

II only

d)

II and III only

115.
What is the equation and cell potential?
a)
2Al3+ + 3Ni → 2Al + 3Ni2+ EO = 1.89 V
b)
2Al + 3Ni2+ → 2Al3+ + 3Ni EO = 1.89 V
c)
2Al3+ + 3Ni → 2Al + 3Ni2+ EO = 1.43 V
d)
2Al + 3Ni2+ → 2Al3+ + 3Ni EO = 1.43 V
116.
This electrode in a voltaic cell loses mass 
a)
Anode
b)
Cathode
117.
In a voltaic cell, the half cell that receives cations from the salt bridge is
a)
Cathode
b)
Anode
118.

What is an anode?

a)

It is the electrode where oxidation takes place.

b)

It is the electrode where reduction takes place.

c)

It is an aqueous solution containing an electrode.

d)

It is the salt bridge that connects half-cells.

119.

What does Ecell need to be for a galvanic cell (thermodynamically favored)?

a)

+

b)

-

120.

If a reaction occurs, then delta G is

a)

negative

b)

positive

c)

can't tell

d)

0

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