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APOADVANCED
PLACEMENT
PROCRAM'
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SECTION IS FOR THE SURVEY QUESTIONS IN THE AP STUDENT PACK. (DO NOT F'UT RESPONSES TO
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EXA';1 QUESTIONS IN THIS SECTION.) BE SURE EACH MARK IS DARK AND COMPLETELY FILLS THE OVAL. '
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DO NOT COMPLETE THIS SECTION UNLESS INSTRUCTED TO DO SO.
R. If this answer sheet is for the French Language, French Literature. German Language, Spanish Language, or Spanish
Literature Examination. please answer the following questions. (Your responses will not affect your grade.)
1. Have you lived or studied for one month or more in a country where the
language of the exam you are now taking is spoken?
<INDICATE YOUR ANSWERS TO THE EXAM QUESTIONS IN THIS SECTION. IF A QUESTION HAS ONLY,FOUR ANSWER
'
n;>P;TlONS, DO NOT MARK OPTioN (E). YOUR ANSWER SHEET Will
BE SCORED BY MACHINE.US(ONI..V:NO.
,?'
) PENCiLS TO MARK YOUR ANSWERS ON PAGES 2 AND 3 (ONE RESPONSE PER. QUESTION). AFTER "OJ.' HAVE,
",DETERMINEDYOUR
RESPONSE, BE SURE TO COMPLETELY FILL IN THE OVAL CORRESPONDING TO THENUrABER OF "
,,~THE QUESTION YOU ARE ANSWERING. STRAY MARKS AND SMUDGES COULD BE READ AS ANSWERS,SO
ERASE .
<CAREFULLY AND COMPLETELY. ANY IMPROPER GRIDDING MAY AFFECT YOUR GRADE.
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FOR QUESTIONS 76-151, SEE PAGE 3.
DO NOT WRITE IN THIS AREA.
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•
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•
Three hours are allotted for this examination. One hour and 30 minutes are allotted for Section 1, which consists of
multiple-choice questions. For Section II, Part A, 40 minutes are allotted; for Section II, Part B, 50 minutes are allotted.
Section I is printed in this examination booklet. Section II is printed in a separate booklet
Time -
1 hour and 30 minutes
Number of questions -75
Percent of total grade -
45
This examination contains 75 multiple-choice questions and 5 survey questions. Therefore, please
be careful to fill in only the ovals that are preceded by numbers 1 through 80 on your answer sheet.
No calculators may be used on this examination.
General Instructions
INDICATE ALL YOUR ANSWERS TO QUESTIONS IN SECTION I ON THE SEPARATE ANSWER SHEET.
No credit will be given for anything written in this examination booklet, but you may use the booklet for notes or
scratchwork. After you have decided which of the suggested answers is best, COMPLETELY fill in the corresponding
oval on the answer sheet. Give only one answer to each question. If you change an answer, be sure that the previous
mark is erased completely.
(A)
(B)
(C)
(D)
(E)
state
city
country
continent
village
Many candidates wonder whether or not to guess the answers to questions about which they are not certain. In this
section of the examination, as a correction for haphazard guessing, one-fourth of the number of questions you answer
incorrectly will be subtracted from the number of questions you answer correctly. It is improbable, therefore, that mere
guessing will improve your score significantly; it may even lower your score, and it does take time. If, however, you are
not sure of the correct answer but have some knowledge of the question and are able to eliminate one or more of the
answer choices as wrong, your chance of getting the right answer is improved, and it may be to your advantage to
answer such a question.
Use your time effectively, working as rapidly as you can without losing accuracy. Do not spend too much time on
questions that are too difficult. Go on to other questions and come back to the difficult ones later if you have time. It is
not expected that everyone yrill be able to answer all the multiple-choice questions.
PERIODIC TABLE OF THE ELEMENTS
1
2
H
He
1.0079
3
4
4.0026
10
Li
Be
6.941
11
9.012
12
Na
Mg
22.99
19
24.30
20
21
22
23
24
K
Ca
Sc
Ti
V
Cr Mn
39.10
37
40.08
38
5
6
B
C
10.811 12.011
13
14
44.96
39
47.90
40
50.94
41
52.00
42
25
54.938
43
7
8
9
N
0
F
Ne
14.007
15
16.00
16
19.00
17
20.179
18
P
S
CI
Ar
Al
Si
28.09
32
30.974
33
32.06
34
35.453 39.948
35
36
26
27
28
29
30
26.98
31
Fe
Co
Ni
Cn
Zn
Ga
Ge
As
Se
Br
Kr
69.72
49
72.59
50
74.92
51
78.96
52
79.90
53
83.80
54
In
Sn
55.85
44
58.93
45
58.69
46
63.55
47
65.39
48
Ag
Cd
Rb
Sr
Y
Zr
Nb
Mo
Tc
Rn
Rh
Pd
85.47
55
87.62
56
88.91
57
91.22
72
92.91
73
95.94
74
(98)
75
lOLl
·76
102.91
77
106.42
78
Cs
Ba
*La Hf
Ta
W
Re
,Os
Ir
Pt
Au
Hg
TI
Pb
Bi
Po
At
Rn
132.91
87
137.33
88
138.91 178.49
89
104
186.21
107
1C)0.2
195.08
110
196.97
111
200.59
112
204.38
207.2
208.98
(209)
(210)
(222)
108
192.2
109
Fr
Ra
(223)
226.02
180.95 183.85
105
106
107.87 112.41
79
80
114.82 118.71
81
82
Sb
Te
I
Xe
121.75
83
127.60
84
126.91
85
131.29
86
tAc Rf
Db
Sg
Bh
Hs
Mt
§
§
§
227.03
(261)
(262)
(263)
(262)
(265)
(266)
(269)
(272)
(277)
58
59
60
61
62
63
64
65
66
67
68
69
70
71
Ce
Pr
Nd
Pm
8m
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
(145)
93
150.4
94
151.97
95
157.25
96
158.93
97
162.50
98
168.93
101
173.04
102
174.97
103
140.12 140.91 144.24
92
90
91
Th
Pa
U
Np
232.04 231.04 238.03 237.05
§Not yet named
164.93 167.26
100
99
Pu Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
(244)
(247)
(247)
(251)
(252)
(257)
(258)
(259)
(260)
(243)
~artA
I
CHEMISTRY
Section I
Time--: 1 hour and 30 minutes
NO CALCULATOR MAYBE USED WITH SECTION I.
Note: For all questions, assume that the temperature is 298 K, the pressure is 1.00 atmosphere, and solutions are
aqueous unless otherwise specified.
T = temperature
P = pressure
V = volume
S = entropy
H = enthalpy
G = Gibbs free energy
R = molar gas constant
n = number of moles
, M= molar
m = molal
L, mL
g
nm
atm
mID Hg
J, kJ
V
mol
=
=
=
=
=
=
=
=
liter(s), milliliter(s)
gram(s)
nanometer(s)
atmosphere(s)
millimeters of mercury
joule(s), kilojoule(s)
volt(s)
mole(s)
Directions: Each set of lettered choices below refers to the numbered statements immediately following it. Select
the one lettered choice that best fits each statement and then fill in the corresponding oval on the answer sheet. A
choice may be used once, more than once, or not at all in each set.
Consider atoms of the following elements. Assume
that the atoms are in the ground state.
(A)
(B)
(C)
(D)
S
Ca
Ga
Sb
(E) Br
1. The atom that contains exactly two unpaired
electrons
2. The atom that contains only one electron in the
highest occup~ed energy sublevel
Unauthorized copying or reuse
of any part of this page is illegal.
(A) CO2
(B) H20
(C) CH4
(D) C2H4
(E) PH3
'
I
~artA
Questions 6-7 refer to the following solid
compounds.
Questions 8-10 refer to the following gases at
and 1 atm.
(A) PbS04
(B)CuO
(A) Ne
(C) KMn04
(C) 02
(D) CO
ooe
(B) Xe
(D) KCl
(E) FeCl3
(E) NO
8. Has an average atomic or molecular speed closest
to that of N2 molecules at aoc and 1 atm
(A) H2SeOiaq)
+ 2 Cl-(aq) + 2 H+(aq) ~ H2Se03(aq)
(B) Ss(s) + 8 02(g) ~
+ Clig)
8 S02(g)
(C) 3 Br2(aq) + 6 OH-(aq)
~
5 Br-(aq) + Br03-(aq)
+ 3 H20(I)
(D) Ca2+(aq)
+ SOl-(aq) ~ CaS04(s)
(E) PtCI4(s) + 2 Cl-(aq) ~ PtCll-:(aq)
13. A reaction in which the same reactant undergoes
both oxidation and reduction
Unauthorized copying or reuse
of any part of this page is illegal.
+ H20(I)
I
~artB
Directions: Each of the questions or incomplete statements below is followed by five suggested answers or
completions. Select the one that is best in each case and then fill in the corresponding oval on the answer sheet.
Questions 15-16 relate to the graph below. The
graph shows the temperature of a pure substance as it
is heated at a constant rate in an open vessel at 1.0
atm pressure. The substance changes from the solid to
the liquid to the gas phase.
.
17. In which of the following groups are the three
species isoelectronic; i.e., have the same number
of electrons?
(A)
(B)
(C)
(D)
(E)
S2-, K+, Ca2+
Sc, Ti, V2+
02-, S2-, ClMg2+, Ca2+, Sr2+
Cs, Ba2+, La3+
I
I
I
I
.-..
I
I
I
I
cd
t2
S
•....
'-'
II)
l-<
t3
Time
15. The substance is at its normal freezing point at
time
(A) t1
(B) t2
(C) t3
(D) t4
(E) t5
16. Which of the following best describes what
happens to the substance between t4 and t5 ?
(A) The molecules are leaving the liquid phase.
(B) The solid and liquid phases coexist in
equilibrium.
(C) The vapor pressure of the substance is
decreasing.
(D) The average intermolecular distance is
decreasing.
(E) The temperature of the substance is
increasing.
Unauthorized copying or reuse
of any part of this page is illegal.
~
VJ
VJ
II)
l-<
D.<
1.5
1.0
0.5
20
40
60
80
Temperature (0C)
100
18. The phase diagram for the pure substance X is
shown above. The temperature of a sample of
pure solid X is slowly raised from lOoC to
lOO°C at a constant pressure of 0.5 atm. What
istl,le expected behavi.or of the substance?
(A) It fITstmelts to a liquid and then boils at about
70°C.
(B) It fITstmelts to a liquid and then boils at about
30°C.
(C) It melts to a liquid at a temperature of about
20°C and remains a liquid until the
temperature is greater than 100°C.
(D) It sublimes to vapor at an equilibrium
temperature of about 20°C.
(E) It remains a solid until the temperature is
greater than lOO°C.
I
~artB
19. In which of the following species does sulfur have
the same oxidation number as it does in_ HZS04 ?
23. Neutron bombardment of uranium can induce Ul••.
reaction represented above. Nuclide X is which
of the following?
(A) HZS03
(B)
SzOl-
(C) Sz-
(A) ~Br
CD) S8
(E) SOzClz
20. A flask contains 0.25 mole of SOz(g), 0.50 mole
of CH4(g), and 0.50 mole of 0zCg). The total
pressure of the gases in the flask is 800 mm Hg.
What is the partial pressure of the S02(g)
in the
flask?
(A)
(B)
(C)
(D)
(E)
800mmHg
600mmHg
250mmHg
200mmHg
160mmHg
.•,...
24. A compound contains 1.10 mol of K,
0.55 mol of Te, and 1.65 mol of 0. What is
the simplest formula of this compound?
(A) KTeO
(B) KTezO
.
21. In the lab0ratory, Hz(g) can be produced by
adding which of the following to 1 M HCl(aq) ?
(C) K2Te03
(D)
KzTe06
(E) K4Te06
I. 1 M NH3(aq)
IT. Zn(s)
ill. NaHC03(s)
(A)
(B)
(C)
(D)
(E)
I only
II only
ill only
I and IT only
I, IT, and ill
25. "W?at i~,the stalldard ~nthalpy change, !:i.H", for
the reaction represented above?
(!:i.H; of CzHzCg) is 230 kJ mol-I;
!:i.H; ofC6~(g)
is 83 kJmol-I.)
(A) -607 kJ
(B) -147 kJ
(C) -19kJ
22. In liquid ammonia, the reaction represented above
occurs. In the reaction NH4 + acts as
(A) a catalyst
(D) +19 kJ
(E) +773 kJ
26. Approximately what mass of CUS04• 5HzO
(B) both an acid and a base
(250 g mol-I) is required to prepare 250 mL
(C) the conjugate acid of NH3
(D) the reducing agent
of 0.10 M copper(II) sulfate solution?
(E) the oxidizing agent
Unauthorized copying or reuse
of any part of this page is illegal.
(A)
4.0 g
(B)
6.2 g
(C) 34 g
(D) 85 g
(E) 140 g
~artB
2 NO(g) + Gig)
-7
2 NOig)
27. A possible mechanism for the overall reaction represented
above is the following.
+ NO(g)
(1)
NO(g)
(2)
N20Z(g)
+
02(g)
-7 NZ02(g)
-7
2 N02(g)
slow
fast
Which of the following rate expressions agrees best with this
possible mechanism?
(A) Rate
=
k[NOf
(B) Rate
=
k
(C) Rate
=
k--
CD) Rate
=
k[NO]2[Oz]
(E) Rate
= k[N20Z][Oz]
~~1
[NO]2
[°2]
Unauthorized copying or reuse
of any part of this page is illegal.
I
21
~artB
I
28. Of the following compounds, which is the most
ionic?
(A) SiCl4
(B) BrCI
(C) PCl3
CD) Cl20
31. What volume of 02(g) is required to react
with excess CS2(1) to produce 4.0 L of CO2 (g) ?
(Assume all gases are measured at O°C and 1 atm.)
(A) 12L
(E) CaCl2
(B) 22.4 L
29. The best explanation for the fact that diamond is
extremely hard is that diamond crystals
(A) are made up of atoms that are intrinsically
hard because of their electronic structures
(B) consist of positive and negative ions that are
strongly attracted to each other .
(C) are giant molecules in which each atom forms
strong covfl.lent bonds with all of its
neighboring atoms
(D) are formed under extreme conditions of
temperature and pressure
(E) contain orbitals or bands of delocalized
electrons that belong not to single atoms but
to each crystal as a whole
(C)
j. x 22.4 L
(D) 2 x 22.4 L
(E)
3 x 22.4 L
32. Which of the following oxides is a gas at 25°C
and 1 atm?
(A) Rb20
(B) N20
(C) Na202
CD) Si02
(E) La203
30. At 25°C, aqueous solutions with a pH of 8 have a
hydroxide ion concentration, [OH-], of
(A) 1 x 10-14 M
(B) 1 x 10-8 M
(C) 1 X 10-6 M
(D) 1 M
(E) 8M
Unauthorized copying or reuse
of any part of this page is illegal.
~artB
The graph below shows the titration curve that
results when 100. mL of 0.0250 M acetic acid is
titrated with 0.100 M NaOH.
14.0
?
12.0
10.0
pH 8.0
6.0
4.0
2.0
0.0 0
-
,....
I
;,
X
-
V
Wj
5 10 15 20 25 30 35 40 45
mL of 0.100 M NaOH Added
35. A solution is made by dissolving a nonvolatile
solute in a pure solvent. Compared to the pure
solvent, the solution
(A)
(B)
(C)
(D)
(E)
has a higher normal boiling point
has a higher vapor pressure
has the same vapor pressure
has a higher freezing point
is more nearly ideal
36. A sample of a solution of an unknown was treated
with dilute hydrochloric acid. The white precipitate
formed was filtered and washed with hot water.
A few drops of potassium iodide solution were
added to the hot water filtrate and a bright yellow
precipitate was produced. The white precipitate
remaining on the filter paper was readily soluble
in ammonia solution. What two ions could have
been present in the unknown?
(A) Ag+(aq) and Hgl+(aq)
33. Which of the following indicators is the best choice
for this titratio~7
pH Range of
Color Change
(A)
(B)
(C)
(D)
(E)
Methyl orange
Methy Ired
Bromothymol blue
Phenolphthalein
Alizarin
3.2 - 4.4
4.8 - 6.0
6.1- 7.6
8.2 -10.0
11.0 - 12.4
34. What part of the curve corresponds to the optimum
buffer action for the acetic acid/acetate ion pair?
(A) Point V
(B) Point X
(C) Point Z
CD) Along all of section WY
(E) Along all of section yz
Unauthorized copying or reuse
of any part of this page is illegal.
I
(B) Ag+(aq) and Pb2+(aq)
(C) Ba2+(aq) and Ag+(aq)
(D) Ba2+(aq) and Hgl+(aq)
(E) Ba2+(aq) and Pb2+(aq)
!
~artB
37. When the reaction represented by the equation above is at equilibrium at 1 atm and 25°C, the ratio
[CO
[
3
] can be increased by doing ;Vhich of the following?
HC03-
2-]
(A)
(B)
(C)
(D)
(E)
Decreasing the temperature
Adding acid
Adding a catalyst
Diluting the solution with distilled water
Bubbling neon gas through the solution
38. A 0.10 M aqueous solution of sodium sulfate,
Na2S04, is a better conductor of electricity than
a 0.10 M aqueous solution of sodium chloride,
NaCl. Which of the following best explains this
observa~on?
(A) NaZS04 is more soluble in water than
NaCI is.
(B) NaZS04 has a higher molar mass than
NaCl has.
(C) To prepare a given volume of 0.10 M
solution,. the mass of NaZS04 needed is
more than twice the mass of NaG neooed.
(D) More moles of ions are present in a given
volume of 0.10 M NaZS04 than in the
same volume of 0.10 M NaCl.
(E) The degree of dissociation of NaZS04 in
solution is significantly greater than that
of NaCl.
Unauthorized copying or reuse
of any part of this page is illegal.
~.
.--- /
'i:'
/
~
~ 160
~
K2S04
00
o
o
:: 120
/
o
0..
/KN03
8
::l
..o
-......
o
<I)
80
'-"
.0
.E 40
o
CI)
/
-----
/
00
-
----10
20
./
.r
.--"
/
NaCI..,.L..
-
~~
K2Cr04-
CeiS04)3
-,I
30
40 50 60 70
Temperature CCc)
80
90
100
39. On the basis of the solubility curves shown above, the greatest
percentage of which compound can be recovered by cooling a
saturated solution of that compound from 90°C to 30°C ?
(A) NaCI
(B) KN03
(C) K2Cr04
(D) K2S04
(E) Ce2(S04)3
Unauthorized copying or reuse
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Part B
I
I
~artB
40. An excess of Mg(s) is added to 100. mL of
0.400 M HCl. At
and 1 atm pressure, what
volume of Hz gas can be obtained?
aoc
(A) 22.4 rnL
(B) 44.8 rnL
(C) 224mL
(D) 448 mL
(E) 896 mL
41. When solid NH4SCN is mixed with solid
Ba(OH)z in a closed container, the temperature
drops and a gas is produced. Which of the following indicates the correct signs for f!.G, MI,
and
/)$
for the process?
f!.G
(A)
(B)
(C)
-
(D)
(E)
+
temperature, the value of the
constant, K, for the reaction
above is 2.0 X lOs. What is the
for the reverse reaction at the same
temperature?
(A) -2.0 x lO-s
(B) 5.0 x 10-6
(C)
(D)
(E)
(A)
(B)
(C)
(D)
(E)
90%
70%
50%
25%
10%
44. Which of the following properties generally
decreases across the periodic table from sodium
to chlorine?
(A)
(B)
(C)
(D)
(E)
First ionization energy
Atomic mass
Electronegativity
Maximum value of oxidation number
Atomic radius
45. What is the
an aqueous
mass? (The
molar mass
+ _.
42. At a certain
equilibrium
represented
value of K
43. The atomic mass of copper is 63.55. Given that
,
there are only two naturally occurring isotopes
copper, 63Cu and 6SCu, the natural abundance of
the 6SCu isotope must be approximately
2.0 X lO-s
5.a x lO-s
5.0 x 10-4
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(A)
(B)
(C)
(D)
(E)
mole fraction of ethanol, CzHsOH, in
solution that is 46 percent ethanol by
molar mass of CzHsOH is 46 g; the
of HzO is 18 g.)
0.25
0.46
0.54
0.67
0.75
46. The effeCtive nuclear charge ~xperienced by
the outermost electron of Na is different than
the effective nuclear charge experienced by the
outermost electron of Ne. This difference best
accounts for which of the following?
(A) Na has a greater density at standard
conditions than Ne.
(B) Na has a lower fIrst ionization energy
than Ne.
(C) Na has a higher melting point than Ne.
(D) Na has a higher neutron-to-proton ratio
than Ne.
(E) Na has fewer naturally occurring isotopes
than Ne.
~artB
I
47. Which of the following is a correct statement
about reaction order?
(A) Reaction order can only be a whole number.
(B) Reaction order can be determined only from
the coefficients of the balanced equation for
the reaction.
(C) Reaction order can be determined only by
experiment.
(D) Reaction order increases with increasing
temperature.
(E) A second-order reaction must involve at least
two different compounds as reactants.
48. Sodium chloride is LEAST soluble in which of
the following liquids?
(A) H20
(B) CC14
(C) HF
(D) CH30H
(E) CH3COOH
49. When the equation above is correctly balanced and all coefficients are redi:lced to lowest whole-number terms,
the coefficient for H+(aq) is
(A)
(B)
(C)
2
4
6
(D) 8
(E) 14
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I
~artB
50. Which of the following represents acceptable
laboratory practice?
(A) Placing a hot object on a balance pan
(B) Using distilled water for the [mal rinse of a
buret before filling it with standardized
solution
(C) Adding a weighed quantity of solid acid to
a titration flask wet with distilled water
(D) Using 10 rnL of standard strength
phenolphthalein indicator sol~tion for
titration of 25 rnL of acid solution
(E) Diluting a solution in a volumetric flask to
its [mal concentration with hot water
51. True statements
about the reaction represented above include which of the following?
..,.1. Cti{s) acts as an oxidizing agent.
II. The oxidation state of nitrogen changes from +5 to +2.
III. Hydrogen ions are oxidized to form H20(l).
(A)
(B)
(C)
(D)
(E)
I only
II only
III only
I and II
II and III
52. Propane gas, ~Hg, burns in excess oxygen gas.
When the equation for this reaction is correctly
balanced and all coefficients are reduced to their
lowest whole-number
02 is
(A) 4
(B) 5
(C) 7
(D) 10
(E) 22
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terms, the coefficient for
~artB
53. According to the VSEPR model, the progressive
decrease in the bond angles in the series of
molecules CH4, NH3• and H20 is best
accounted for by the
(A) increasing strength of the bonds
(B) decreasing size of the central atom
(C) iricreasing electronegativity of the central
atom
(D) increasing number of unshared pairs of
electrons
(E) decreasing repulsion between hydrogen
atoms
54. Which of the following must be true for a reaction
for which the activation energy is the same for
both the forward and the reverse reactions?
(A) A catalyst is present.
(B) The reaction order can be obtained directly
from the balanced equation.
(C) The reaction order is zero.
(D) ~H for the reaction is zero.
(E) ~s for the reaction is zero.
Time (days)
% Reactant
remaining
0
100
1
79
2
63
3
50
4
40
5
31
6
25
7
20
10
.. 0.
.
10
. ..
20
1
55. A reaction was observed for 20 days and the percentage of the reactant remaining after each day
was recorded in the table above. Which of the following best describes the order and the half-life
of the reaction?
Reaction Order
(A)
(B)
(C)
(D)
(E)
First
First
Second'
Second
Second
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Half-life (days)
3
10
3
6
10
I
I
~arlB
56. The boiling points of the elements h.elium, neon,
argon, krypton, and xenon increase ill that order.
Which of the following statements accounts for
this increase?
(A)
(B)
(C)
(D)
(E)
The
The
The
The
The
London (dispersion) forces increase.
hydrogen bonding increases.
dipole-dipole forces increase.
chemical reactivity increases.
number of nearest neighbors increases.
58. When 8.0 g of N2H4 (32 g mol-I) and 92 g of
N204 (92 g mol-I) are mixed together and react
according to the equation above, what is the
maximum mass of H20 that can be produced?
(A)
9.0 g
(B)
(C)
18g
36 g
(D)
72 g
(E) 144g
57. The rate of a certain chemical reaction between
substances M and N obeys the rate law above.
The reaction is fIrst studied with [M] and [N]
each 1 x 10-3 molar. If a new experiment is
10-3
conducted with [M] and [NJ each 2 x
molar, the reaction rate will increase by a factor of
(A)
2
(B)
4-'
(C) 6~;
(D) 8
(E) 16
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59. All of the halogens in their elemental form at
25°C and 1 atm are
(A)
(B)
(C)
(D)
(E)
conductors of electricity
diatomic molecules
odorless
colorless
gases
~artB
60. According to the balanced equation above, how many moles of Cl02-(aq) are needed to react completely with
20. mL of 0.20 M KMn04
(A)
(B)
(C)
(D)
(E)
solution?
0.0030 mol
0.0053 mol
0.0075 mol
0.013 mol
0.030 mol
61. How can 100. mL of sodium hydroxide solution
with a pH of 13.00 be converted to a sodium
hydroxide solution with a pH of 12.00 ?
.,
Unauthorized copying or reuse
of any part of this page is illegal.
(A) By diluting the solution with distilled water
to a total volume of 108 mL
(B) By diluting the solution with distilled water
to a total volume of 200 mL
(C) By diluting the solution with distilled water
to a total volume of 1.00 L
(D) By adding 100. mL of 0.10 M HCl
(E) By adding 100. mL of 0.10 M NaOH
~artB
H
H
I
H-C-C-C-Br
1
I
H
63. Mixtures that would be considered buffers include
which of the following?
..
H
1
I'
I.O.I0MHCI+O.I0MNaCI
II.O.I0MHF+0.lOMNaF
m.O.lOMHBr+0.l0MNaBr
I
H
H
62. Which of the following structural formulas
represents an isomer of the compound that has
the structural formula represented above?
H
H
I
I
I
I
H
I
I
Br-C-C-C-H
H
I only
II only
monly
I and II
II and m
64. Ascorbic acid, H2C6~06(s), is a diprotic acid
with K = 7.9 X 10-5 and K = 1.6 X 10-12.
H H H
H
(A)
(B)
(C)
(D)
(E)
1
2
In a 0.005 M aqueous solution of ascorbic acid,
which of the following species is present in the
H
I I I
H-C-C-C-H
I I I
lowest concentration?
I
H' Br
(A) H20(l)
H
H H H
~'I
,I
I
I
H
H
H--C-C-C-H
I
I .
Br
I
I
I
I
(D) HC6~06 -(aq)
(E) C6~Oi-(aq)
65. Which of the foJ)owing substances is LEAST
soluble in water?
H H H
Br-C-C-C-Br
(B) H30+(aq)
(C) H2C6~06(aq)
I
I
(A) (NH4)2S04
(B) KMn04
H H H
.
(C) BaC03
H H H H
I I I
H-C-C-C-C-Br
I I I
H
H
H
I
I
H
(D) Zn(N03h
(E) Na3P04
66. A 2 L container will hold about 4 g of which of
the following gases at O°Cand 1 a1m?
(A) S02
(B) N2
(C) CO2
(D) C4Hg
(E) NH3
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of any part of this page is illegal.
~artB
67. Which of the following describes the changes in
forces of attraction that occur as H20 changes
phase from a liquid to a vapor?
(A) H-O bonds break as H-H and 0-0
bonds form.
(B) Hydrogen bonds between H20 molecules
are broken.
(C) Covalent bonds between H20 molecules are
69. If 200. mL of 0.60 M MgCI2(aq)
is added
to 400. mL of distilled water, what is the
concentration of Mg2+(aq) in the resulting
solution? (Assume volumes are additive.)
(A) 0.20M
(B)
0.30M
(C) OAOM
(D) 0.60M
(E) 1.2M
broken.
(D) Ionic bonds between H+ ions and OHions are broken.
(E) Covalent bonds between H+ ions and H20
molecules become more effective.
70. Of the following pure substances, which has the
highest melting point?
(A) S8
(B) 12
(C) Si02
(D)
100
S02
(E) C6~
90
71. In the electroplating of nickel, 0.200 faraday of
electrical charge is passed through a solution of
NiS04• What mass of nickel is deposited?
"""' 80
u
~
•...
0
70
(A)
2.94 g
(B)
5.87 g
(C) 11.7 g
(D) 58.7 g
(E) 294 g
~ 60
~
S' 50
0
Eo-<
40
30
20
0
1
2
3
4
5
6
7
Time (minutes)
72. A colorless solution is divided into three samples.
The following tests were performed on samples of
the solution.
.
Sample
68. Liquid naphthalene at 95°C was cooled to 30°C,
as represented in the cooling curve above. From
which section of the curve can the melting point
of naphthalene be determined?
(A) A
(B) B
(C) C
(D) D
(E)E
Observation
1
Add H+(aq)
No change
2
Add NH3(aq)
No change
3
Add SOl-(aq)
No change
Which of the following ions could be present in
the solution at a concentration of 0.10 M ?
(A) Ni2+(aq)
(B) Al3+(aq)
(C) Ba2+(aq)
(D) Na+(aq)
(E) COl-(aq)
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Test
I
~artB
75. In a saturated solution of Zn(OHh
73. Which of the following is true for any substance
undergoing the process represented above at its
normal melting point?
(A) JiS <
(B) JiB
(C) JiB
(D) TJiS
(E) JiB
0
=0
= TJiG
=0
= TJiS
74. A pure, white crystalline solid dissolves in water
to yield a basic solution that liberates a gas when
excess acid is added to it. On the basis of this
information, the solid could be
(A) KN03
(B) K2C03
I
(C) KOH
(D) KHS04
(E) KCt.
Unauthorized copying or reuse
of any part of this page is illegal.
at 25°C, . -:.\
the value of [OH-] is 2.0 x 10-6 M. What is
value of the solubility-product
.
Zn(OH)2 at 25°C?
(A) 4.0 x 10-18
(B) 8.0 X 10-18
(C) 1.6 X 10-17
(D) 4.0 X 10-12
(E) 2.0 X 10-6
constant, K
~'
ihe';
for
For a given range of multiple-choice
If you have calculated
scores, this table shows the percentage
the mulriple-choice
of students
Table 4.2, you can use this table to figure out the most likely grade that the student
that mulriple-choice
score.
receiving each AP grade.
score (Weighted Section I Score) by using the formula shown in
would receive based only on
If you give your students the 2002 exam for practice, you may want to analyze their results to find overall strengths
and weaknesses in their understanding
of AP Chemistry. The following diagnostic worksheet will help you do this;
feel free to photocopy and distribute it to your students for completion.
1.
In each section, students should insert a check mark for each correct answer.
2.
Add together the total number of correct answers for each section.
3.
Compare the student's number of correct answers for each section with the average number correct
for that section.
In addition, under each item, the percent of AP students who answered correctly is shown, so students can analyze
their performance on individual items.
This information will be helpful in deciding how students should plan their study time. Please note that one item
may appear in several different categories, as questions can cross over different topics.
Question #
I
1
2
17
19
43
44
46
63
70
70
72
49
70
62
3
4
5
28
29
53
56
67
54
75
68
51
62
62
52
Correct/Incorrect
Percent of students
answering correctly.
Question #
Correct/Incorrect
Percent of students
anSwering correctly.
74
""
~;
.
. ~.;~..
Structure of Matter/Nuclear"Chemistry
Question #
(Average number correct': 0.4 ·out of 1)
23
Correct/Incori-e"~t
Percent of students
answering correctly.
Question #
37
8
9
10
20
31
66
41
71
59
67
56
41
Correct/Incorrect
Percent of students
answering correctly.
15
16
18
68
Percent of students
answering correctly.
56
58
69
51
Question #
26
35
38
39
45
48
61
69
Percent of students
answering correctly.
56
53
61
13
44 48
22
46
Question #
11
12
13
14
19
22
30
33
51
61
63
71
49
22
25
13
Question #
CorrectlIncorrect
CorrectlIncorrect
Correct/Incorrect
I
Percent of students
answering correctly.
82
30
61
14
12 51
12
10
Question #
24
31
40
43
49
52
58
60
Percent of students
answering correctly.
82
56
29
49
31
11
41
53
Question #
34
37
42
64
75
Percent of students
answering correctly.
34
45
24
38
21
Question #
27
47
54
55
57
Percent of students
answering correctly.
45
39
43
55
52
Question #
25
41
54
73
66
43
43
34
CorrectlIncorrect
CorrectlIncorrect
CorrectlIncorrect
Correct/Incorrect
Percent of students
answering correctly.
6
Question #
7
21
32
44
62
65
70
74
40
28
45
29
21
59
Co rrect/Inco rrect
-
Percent of students
answering correctly.
55
61
48
69
10
Question #
33
36
50
68
72
Percent of students
answering correctly.
10
28
16
51
35
Question #
20
24
25
26
40
42
43
45
57
58
60
66
69
71
75
61
82
66
56
29
24
49
44
52
41
53
41
46
13
21
Correct/Incorrect
Correct/Incorrect
Percent of students
answering correctly.
,