1. science
2. chemistry

The Washington Professional
Educator Standards Board
Washington Educator Skills Tests
Sample Test Questions
Chemistry
WA-SG-FLD023-02
Washington Educator Skills Tests—Endorsements (WEST–E)
SAMPLE TEST QUESTIONS
The sample test questions in this document are designed to give you an introduction to the nature
of the questions included in the Washington Educator Skills Tests—Endorsements (WEST–E).
They represent the various types of questions you may expect to see on an actual test in this test
field; however, they are not designed to provide diagnostic information to help you identify specific
areas of individual strength or weakness or to predict your performance on the test as a whole.
Work through the sample questions carefully before referring to the answer key that follows. The
answer key provides the correct response for each question and lists the objective within the test
framework to which each question is linked. When you are finished with the sample questions, you
may wish to review the test objectives and descriptive statements provided in the test framework for
this test field.
In addition to reading and answering the sample questions, you should also utilize the following
preparation materials available on the WEST Web site:

Read WEST–E Test-Taking Strategies to understand how test questions are designed to
measure specific test objectives and to learn important test-taking strategies for the day of the
test.

Review the Test Summary and Framework for your test field to familiarize yourself with the
structure and content of the test. This document contains general testing information as well as
the percentage of the total test score derived from each content domain described in the test
framework.
Please note that a periodic table, a set of constants, and a set of formulas are provided for this
test. Please refer to these materials as needed in responding to the sample test questions.
These materials are located in the Reference Materials section at the end of this document.
A scientific calculator may be used for this test as needed in responding to the sample test
questions, and one will be provided at the test administration. Please refer to the current WEST
registration information regarding the use of calculators at the test administration.
Readers should be advised that this document, including many of the excerpts used herein,
is protected by federal copyright law.
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—1—
SAMPLE TEST QUESTIONS
Chemistry
SAMPLE MULTIPLE-CHOICE QUESTIONS
1.
A chemist has determined that an
unknown sample has a high melting point,
is ductile, and forms hydrogen gas and a
salt when reacted with HCl acid. Based
on these findings, the unknown sample is
also likely to:
A.
2.
3.
Rutherford's gold foil experiment
provided evidence that led to which of
the following conclusions about atomic
structure?
A.
Electrons exist only in certain
discrete energy levels.
B.
Atoms contain small densely packed
nuclei.
C.
The exact location of an electron
at any given time cannot be
determined.
D.
Atoms display the properties of both
particles and waves.
have a high electronegativity value.
B.
be brittle at room temperature.
C.
have a dull appearance.
D.
be a good conductor of electricity.
In which of the following sets of elements
are the elements arranged in order of
increasing atomic radius?
A.
Po, Sb, Ge
B.
Li, Na, K
C.
Si, P, S
D.
Br, Cl, F
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—2—
SAMPLE TEST QUESTIONS
Chemistry
4.
Use the reactions below to answer the
question that follows.
235
92U
236
92U
+ 10n
A
A
141
56Ba
6.
Use the diagram below to answer the
question that follows.
Phase Diagram for a Compound
236
92U
500
1
+ 92
36K + 3 0n
400
5.
A.
the medical treatment of cancer
B.
the dating of archaeological artifacts
C.
the production of electricity
D.
the irradiation of food products
Ethanol has a specific heat of 2.45 J/g•K
and a density of 0.7893 g/cm3. How much
heat is required to raise the temperature
of 100.0 mL of ethanol from 5.0°C to
20.0°C?
A.
2.90 kJ
B.
3.68 kJ
C.
55.7 kJ
D.
70.6 kJ
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300
Pressure (mm Hg)
The reactions described in the equations
above are used in which of the following
applications?
200
100
50
40
30
20
10
0
–25
X
0
25
50
75
Temperature (°C)
100
Which of the following changes will lead
to the sublimation of the sample at point X
on the phase diagram above?
A.
increasing the pressure to
500 mm Hg
B.
decreasing the temperature to
–5.0°C
C.
increasing the temperature to
100.0°C
D.
decreasing the pressure to 5 mm Hg
—3—
SAMPLE TEST QUESTIONS
Chemistry
7.
Use the information below to answer the question that follows.
A
2CuO(s) + 2H2(g)
1
Cu(s) + 2 O2(g)
1
H2(g) + 2 O2(g)
2Cu(s) + 2H2O(B)
A
CuO(s) ΔH°f = –156.1 kJ/mol
A
H2O(B) ΔH°f = –285.8 kJ/mol
Given the balanced equations and standard
molar enthalpies of formation shown
above, what will be the standard enthalpy
° ) for the reaction between
change (ΔHrxn
copper oxide and hydrogen?
A.
–259.4 kJ
B.
–441.9 kJ
C.
–883.8 kJ
D.
–1320 kJ
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—4—
SAMPLE TEST QUESTIONS
Chemistry
8.
Use the table below to answer the question that follows.
Molecule
Molecular
Geometry
Molecular
Polarity
CH4
trigonal pyramidal
polar
CO2
linear
nonpolar
NH3
tetrahedral
polar
H2O
bent
nonpolar
In the table above, which molecule is
matched with its correct molecular
geometry and molecular polarity?
A.
CH4
B.
CO2
C.
NH3
D.
H2O
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—5—
SAMPLE TEST QUESTIONS
Chemistry
9.
Use the table below to answer the question that follows.
Line
Chemical Formula
IUPAC Name
1
Fe2O3
iron(II) trioxide
2
CH3CO2
methylcarbonate ion
3
CH3CH2CH3
propane
4
PCl5
phosphorus chloride
–
Which line in the table above correctly
matches a chemical formula with its
IUPAC name?
A.
Line 1
B.
Line 2
C.
Line 3
D.
Line 4
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—6—
SAMPLE TEST QUESTIONS
Chemistry
10.
Use the equation below to answer the question that follows.
Ca(OH)2(s) + H2SO4(aq)
A
CaSO4 • 2H2O(s)
The equation above describes a process
commonly used by coal-fueled power
plants to remove sulfur oxides present in
exhaust gases. This is an example of
which of the following types of chemical
reactions?
A.
combustion
B.
single replacement
C.
neutralization
D.
decomposition
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—7—
SAMPLE TEST QUESTIONS
Chemistry
11.
Use the information below to answer the question that follows.
Reaction of Nitrogen Dioxide and Carbon Monoxide
overall reaction: NO2(g) + CO(g)
A
NO(g) + CO2(g)
step 1 of reaction mechanism: NO2(g) + NO2(g)
A
NO3(g) + NO(g)
At low temperatures, the reaction between nitrogen dioxide and carbon monoxide occurs in two steps.
Given the information shown above, which of the following reactions is step 2 of the reaction
mechanism?
A.
NO3(g) + NO(g)
A
N2O4(g)
B.
NO3(g) + CO(g)
A
NO2(g) + CO2(g)
C.
NO(g) + NO2(g)
A
2NO(g)
D.
NO(g) + CO(g)
A
N(g) + CO2(g)
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—8—
SAMPLE TEST QUESTIONS
Chemistry
12.
Use the reaction below to answer the
question that follows.
N2(g) + 3H2(g) f 2NH3(g)
The Haber-Bosch process used in the
commercial synthesis of ammonia from
nitrogen and hydrogen is shown above.
The process includes a condensation step
in which the ammonia gas produced is
condensed into a liquid. Which of the
following best describes the role this
condensation step plays in the process?
A.
Reducing the concentration of
ammonia gas shifts the equilibrium
to the right, driving the formation of
more product.
B.
Removing ammonia gas from the
system lowers the activation energy
of the synthesis reaction.
C.
Condensing the ammonia gas
into its liquid state removes
contaminants that may have been
introduced into the system.
D.
Converting ammonia gas to a liquid
increases the equilibrium constant,
leading to a greater yield of product.
13.
Use the information below to answer
the question that follows.
2Fe3+(aq) + 2I –(aq) A
Standard Reduction Potentials
(at 25°C)
Half-reaction
Fe3+(aq) + e–
I2(s) + 2e–
A
A
Fe2+(aq)
2 I–(aq)
E°(V)
0.769
0.534
The net ionic equation for the reaction
between iron(III) ions and iodide ions and
the standard reduction potentials for the
related half-reactions are shown above.
Given the value for the Faraday constant
of F = 9.648 × 104 J/mol•V, what will be
the standard free-energy change (ΔG°) for
this reaction at 25°C?
A.
–22.7 kJ
B.
–45.3 kJ
C.
–90.6 kJ
D.
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2Fe2+(aq) + I2(s)
–251 kJ
—9—
SAMPLE TEST QUESTIONS
Chemistry
14.
Use the diagrams below to answer the
question that follows.
C
Use the table below to answer the
question that follows.
H
H
NH2
15.
COOH
H
NH2
C
Ascorbic Acid
(molar mass = 176.1 g/mol)
COOH
CH2
OH
Percent by Mass
of Component
Elements
Component
Elements of
Ascorbic Acid
54.5
oxygen
40.9
carbon
4.6
hydrogen
The two amino acids shown above can
be joined together using which of the
following chemical reactions?
A.
esterification
B.
substitution
C.
combustion
D.
condensation
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The table above gives the molar mass
of ascorbic acid and the percent by mass
of its component elements. Given this
information, what is the molecular
formula for ascorbic acid?
A.
C3H4O3
B.
C6H6O6
C.
C9H12O9
D.
C6H8O6
—10—
SAMPLE TEST QUESTIONS
Chemistry
16.
Use the reaction below to answer the
question that follows.
CO(g) + 2H2(g)
A
CH3OH(B)
534 g CO and 98.0 g H2 are combined to
form methanol according to the reaction
above. What mass of the excess reactant
remains after all of the limiting reactant
has been consumed?
A.
21.2 g
B.
59.7 g
C.
98.2 g
D.
338 g
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17.
Scuba divers that surface too quickly
after spending time at depths greater than
15 m need to take precautions during their
ascent to prevent the formation of nitrogen
gas bubbles in the bloodstream. This
problem experienced by divers is most
similar to which of the following physical
phenomena?
A.
The boiling point of water is
increased by dissolving table salt
in the water.
B.
The air molecules in a balloon
expand the volume of the balloon as
it rises into the atmosphere, where
atmospheric pressure is lower.
C.
The adiabatic warming of an
air mass occurs as the air is
compressed.
D.
The dissolved carbon dioxide in
soda comes out of solution when the
pressure is decreased as the bottle is
opened.
—11—
SAMPLE TEST QUESTIONS
Chemistry
18.
Use the chart below to answer the question that follows.
Emissions Data for Four Experimental Fuel Additives
additive 1
Emissions (as a percent of control)
100
90
additive 2
80
70
60
50
additive 3
40
30
additive 4
20
10
0
0
10
20
30
40
Speed (mph)
50
60
A research chemist has synthesized four fuel additives designed to reduce auto emissions. The
experimental fuel additives were added to commercial gasoline and emissions data were collected for
speeds ranging from 5 mph to 65 mph. The collected data were graphed in the above chart to show the
effectiveness of each additive at different speeds. Which of the following conclusions is best supported
by the results shown in the chart?
A.
Additive 1 demonstrates the greatest increase in fuel efficiency over the widest range of driving
speeds.
B.
Additives 2 and 4 have the same effect on emissions if all driving speeds are considered.
C.
Additive 4 is most effective at reducing emissions at speeds greater than 50 mph.
D.
Additive 3 produces the greatest average reduction in emissions when all driving speeds are
considered.
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—12—
SAMPLE TEST QUESTIONS
Chemistry
19.
Read the newspaper article below; then answer the question that follows.
New Energy Source Could End Country's Reliance on Fossil Fuels
By providing abundant and clean energy, a newly discovered fusion process promises to
dramatically reduce the country's reliance on fossil fuels. Researchers at a leading university
announced that they have succeeded in producing abundant energy through a relatively
inexpensive fusion process. With the world's reliance on fossil fuels implicated as a major
cause of global warming, many people have proclaimed the discovery as one of the most
important of our time. The researchers who worked on the project said that many existing
power plants could be retrofitted with the new technology, reducing both the environmental
and political problems associated with the country's dependence on fossil fuels.
The newspaper article shown above
describes the discovery of a new process
for producing energy. In evaluating
whether the researchers' claims about this
fusion process are valid, which of the
following questions is it most important
to consider?
A.
Have the researchers released
information on the source of funds
used to develop the process?
B.
Will the process announced by
the researchers provide affordable
energy to the average consumer?
C.
Have the researchers' claims about
the process been evaluated by
scientists not connected to the
project?
D.
Will the raw materials required to
carry out the process be available
to underdeveloped countries?
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—13—
SAMPLE TEST QUESTIONS
Chemistry
20.
Use the diagram below to answer the question that follows.
H2SO4 and water solution
6 V battery
A scientist plans to set up and use the
apparatus shown in the diagram above to
decompose water by electrolysis. Which
of the following aspects of setting up and
using this apparatus represents the most
serious safety hazard?
A.
the removal of insulation from the
ends of the wires
B.
the addition of sulfuric acid to the
water in the beaker
C.
the connection of the wires to the
terminals of the 6 V battery
D.
the displacement of water within the
inverted test tubes
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—14—
SAMPLE TEST QUESTIONS
Chemistry
ANSWER KEY
Question
Number
Correct
Response
Test
Objective
1
D
0001
2
B
0002
3
B
0003
4
C
0004
5
A
0005
6
D
0006
7
A
0007
8
B
0008
9
C
0010
10
C
0011
11
B
0012
12
A
0013
13
B
0014
14
D
0016
15
D
0017
16
A
0018
17
D
0019
18
D
0020
19
C
0021
20
B
0022
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—15—
SAMPLE TEST QUESTIONS
Chemistry
REFERENCE MATERIALS
Please use the reference materials on the following pages as needed in responding to the sample
test questions. These materials will also appear in test booklets.
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Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004
—16—
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—17—
5
15
90
Th
232.0
89
Ac
(227)
Actinide
Series
91
Pa
231.0
59
Pr
140.9
92
U
238.0
93
Np
(237)
94
Pu
(244)
95
Am
(243)
111
96
Cm
(247)
112
97
Bk
(247)
113
98
Cf
(251)
114
99
Es
(252)
115
16
100
Fm
(257)
116
84
Po
(209)
17
101
Md
(258)
117
85
At
(210)
102
No
(259)
118
86
Rn
(222)
54
Xe
131.3
36
Kr
83.8
18
Ar
39.9
10
Ne
20.18
103
Lr
(262)
71
Lu
175.0
53
I
126.9
35
Br
79.9
17
CI
35.5
9
F
19.00
VIIA
70
Yb
173.0
52
Te
127.6
34
Se
79.0
16
S
32.1
8
O
16.00
VIA
69
Tm
168.9
83
Bi
209.0
51
Sb
121.8
33
As
74.9
15
P
31.0
7
N
14.01
VA
68
Er
167.3
82
Pb
207.2
50
Sn
118.7
32
Ge
72.6
14
Si
28.1
67
Ho
164.9
81
TI
204.4
49
In
114.8
31
Ga
69.7
66
Dy
162.5
80
Hg
200.6
48
Cd
112.4
30
Zn
65.4
IIB
65
Tb
158.9
79
Au
197.0
47
Ag
107.9
29
Cu
63.5
IB
64
Gd
157.3
110
Ds
(271)
78
Pt
195.1
46
Pd
106.4
28
Ni
58.7
63
Eu
152.0
109
Mt
(268)
77
Ir
192.2
45
Rh
102.9
27
Co
58.9
VIIIB
62
Sm
150.4
108
Hs
(277)
76
Os
190.2
44
Ru
101.1
26
Fe
55.8
61
Pm
(145)
107
Bh
(264)
75
Re
186.2
43
Tc
(98.9)
25
Mn
54.9
VIIB
60
Nd
144.2
106
Sg
(266)
74
W
183.9
42
Mo
95.9
24
Cr
52.0
VIB
13
AI
27.0
6
C
12.01
IVA
Some of the elements 111 and above have been reported but not fully authenticated and named.
58
Ce
140.1
105
Db
(262)
57
La
138.9
104
Rf
(261)
73
Ta
180.9
41
Nb
92.9
23
V
50.9
Lanthanide
Series
89–103
72
Hf
178.5
40
Zr
91.2
22
Ti
47.9
VB
88
Ra
(226)
57–71
39
Y
88.9
21
Sc
45.0
IVB
IIIB
87
Fr
(223)
12
56
Ba
137.3
11
55
Cs
132.9
10
38
Sr
87.6
9
37
Rb
85.5
8
20
Ca
40.1
7
19
K
39.1
4
12
Mg
24.3
11
Na
23.0
3
4
Be
9.01
3
Li
6.94
5
B
10.81
IIIA
IIA
6
14
2
He
4.00
13
2
VIIIA
IA
1
H
1.01
18
1
PERIODIC TABLE OF THE ELEMENTS
CONSTANTS
Description
Value
Avogadro's number
6.02 × 1023/mol
Molar gas volume at STP
22.4 L
Ideal gas constant (R)
0.0821 L•atm/mol•K = 8.31 J/mol•K
Molal freezing point depression constant for water (Kf)
1.86°C/m
Molal boiling point elevation constant for water (Kb)
0.52°C/m
Heat of fusion of water (ΔHfus)
334 J/g = 80 cal/g
Heat of vaporization of water (ΔHvap)
2260 J/g = 540 cal/g
Specific heat (s) of liquid water
4.18 J/g•°C = 1.0 cal/g•°C
Specific heat (s) of water vapor
2.09 J/g•°C = 0.50 cal/g•°C
Specific heat (s) of solid water
2.11 J/g•°C = 0.50 cal/g•°C
Standard atmospheric pressure (STP)
101.325 kPa = 760 mm Hg
Planck's constant (h)
6.63 × 10– 34 J•s
Speed of light in a vacuum (c)
3.00 × 108 m/s
Dissociation constant of water (Kw)
1.0 × 10– 14 at 25°C
FORMULAS
Description
Formula
Ideal gas law
PV = nRT
Gibbs free energy equation
ΔG = ΔH – TΔS
Free energy of a redox reaction
ΔG° = –nFE°
Root-mean-square speed
urms =
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3RT
M
—18—
FORMULAS (continued)
Description
Formula
Photon energy
E = hν
Speed of light
c = λν
Amount of heat (q)
q = msΔT
Boyle's and Charles' laws combined
P1V1 P2V2
T1 = T2
Graham's law of diffusion
r1
r2 =
M2
M1
NOTES FOR CHEMISTRY TEST
Not all constants and formulas necessary are listed, nor are all constants and formulas listed used on this test.
While attention has been paid to significant figures, no answer should be considered incorrect solely because of
the number of significant figures.
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Evaluation Systems, Pearson, P.O. Box 226, Amherst, MA 01004
—19—