Download AP Chemistry Placement Test To be successful in AP Chemistry

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AP Chemistry Placement Test
To be successful in AP Chemistry, students need a working knowledge of high school
chemistry and math through Algebra 2. This placement test is a 40 question, multiple-choice
test. The test covers some important math skills and topics covered in the first half of
introductory chemistry such as definitions of elements, compounds, mixtures, atoms, molecules,
ions and types of bonds. Problems involving percentages, density, atomic structure, formulas,
molecular weight, moles, and reaction stoichiometry are included. To pass the test, a minimum
of 32 questions must be answered correctly.
Directions:
This is a closed-book exam. You may use a calculator. Answer each of the following
questions and record your answers. You should take no more than 2-hours to complete it. After
completing the test, prepare a MS Word document that lists the question number and your letter
choice. At the end of your document, cut and paste the following statement, have your parent
read it, and type their name that they agree with it.
“My son or daughter has taken this test under the conditions that were specified. I affirm
that my child independently answered each question, and they did not receive help to
complete the test.”
Signed:
____________________________________
Identify your document using the following format: LastnameFirstnamePtest.doc. Email your
document as an attachment to [email protected].
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General Information: Avogadro’s number is 6.022 x 1023
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1) How many numbers below have 5 significant figures?
0.0054
19.000
0.00006
1.6090 x 108
A. 1
B. 2
C. 3
D. 4
E. 5
2) Which of the following is the smallest mass?
A. 2.1 kg
B. 4.2 x 1010 kg
C. 5.8 x 102 g
D. 8.4 x 104 cg
E. 6.7 x 104 mg
3) Given Z = 0.43 Y + 12, what is Y when Z = 28?
A. 93
B. 6.9
C. 24
D. 17
E. 37
4) How many kilometers is 5.82 x 104 cm?
A. 5.82 x 103 km
B. 0.582 km
C. 5.82 x 109 km
D. 5.82 km
E. 5.82 x 105 km
5) All of the following relationships are true EXCEPT
A.
B.
C.
D.
E.
0.328 g = 328 mg
23 km < 4.5 x 107 mm
0.84 kg > 8.4 x 104 mg
41.3 mL > 8.72 x 10-2 L
1.3 nm = 1.3 x 10-6 mm
13607
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6) Express 0.005390 in exponential notation.
A. 5.390 x 10-3
B. 5.390 x 10-1
C. 5.39 x 10-1
D. 0.5390 x 102
E. 5.39 x 103
7) What is the correct answer to the expression below?
(2.54 cm/inch) x (182.3 inch – 179.219 inch) =
A. 8 cm
B. 7.8 cm
C. 7.83 cm
D. 7.826 cm
E. 7.8257 cm
8) Which is the correct answer to the expression below?
1.472 x 10-7 + 4.32 x 10-9 =
A. 2 x 10-7
B. 1.5 x 10-7
C. 1.52 x 10-7
D. 1.515 x 10-10
E. 1.515 x 10-7
9) How many ounces are contained in a 2.0 L soft drink bottle? (1.0 ounce = 29.6 mL)
A. 0.017 oz
B. 0.068 oz
C. 59 oz
D. 68 oz
E. 1.4 x 102 oz
10) A standard sheet of paper is 8.5 x 11 inches. What is the surface area, in cm2, of one side of
a sheet of paper? (2.54 cm = 1 inch)
A. 14 cm2
B. 37 cm2
C. 94 cm2
D. 240 cm2
E. 6.0 x 102 cm2
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11) How many miles are covered in a 15 km race? (1 mile = 5280 feet, 12 inches = 1 foot, 1 inch
= 2.54 cm)
A. 7.1 mile
B. 9.3 mile
C. 11 mile
D. 15 mile
E. 26 mile
12) The density of silver is 10.5 g/cm3. What volume in cm3 would be occupied by a piece of
silver with a mass of 61.3 g?
A. 0.171
B. 644
C. 10.5
D. 0.00155
E. 5.84
13) How many significant figures should there be in the answer to the following computation?
(10.07 + 7.395)
2.5
A. 1
B. 2
C. 3
D. 4
E. 5
14) What is the percent, by mass, of oxygen in Zn(BrO 3)2?
A. 24.83%
B. 39.00%
C. 29.89%
D. 39.79%
E. 17.57%
15) A metal having a mass of 44 grams is dropped in 118.2 mL of water and sinks to the bottom.
The volume of the water and the metal is 124.3 mL. What is the density of the metal?
A. 0.37 g/mL
B. 7.2 g/mL
C. 0.35 g/mL
D. 2.7 g/mL
E. 2.9 g/mL
16) If 250 mL of a 0.50 M NaCl solution is diluted to 840 mL, what is the molarity of the
resulting solution?
A. 0.15 M
B. 6.7 M
C. 0.60 M
D. 1.7 M
E. 0.0025 M
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17) How many atoms of carbon are in 24 grams of carbon?
A. 1.2 x 1024 atoms
B. 1.7 x 1026 atoms
C. 1.2 x 1025 atoms
D. 3.0 x 1024 atoms
E. 3.0 x 1023 atoms
18) A solution is prepared by dissolving sugar in water. The solution is 25.0% sugar by mass.
How many grams of water are in 472 grams of this solution?
A. 118 g
B. 157 g
C. 408 g
D. 354 g
E. 396 g
19) The balanced chemical equation for the reaction between PCl5 and water is given below. If
3.45 moles of HCl are produced, how many moles of water reacted?
PCl5 + 4 H2O → H3PO4 + 5 HCl
A.
B.
C.
D.
E.
0.690 mol
0.863 mol
2.76 mol
3.45 mol
4.31 mol
20) When the equation N2O5 (g) + H2O (l) → HNO3 (aq) is balanced, the coefficient for nitric
acid is
.
A.
B.
C.
D.
E.
5
2
3
4
1
21) How many grams of AlF3 are in 2.64 moles of AlF3 ?
A.
B.
C.
D.
E.
3.14 x 102 g
121 g
222 g
5.74 x 10-2 g
31.8 g
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22) All phosphorus atoms have the same
A.
B.
C.
D.
E.
atomic number
mass number
number of neutrons plus the number of electrons
number of neutrons plus the number of protons
neutrons
23) Which compound has the greatest percent composition by mass of sulfur?
A.
B.
C.
D.
BaS
CaS
MgS
SrS
24) Which element in the ground state has a stable electron configuration?
A.
B.
C.
D.
carbon
magnesium
neon
oxygen
25) According to the kinetic molecular theory for an ideal gas, all gas particles
A.
B.
C.
D.
are in random, constant, straight-line motion.
are separated by very small distances relative to their sizes.
have strong intermolecular forces.
have collisions that decrease the total energy of the system.
26) The chemical process in which electrons are gained by an atom or an ion is called
A.
B.
C.
D.
addition
oxidation
reduction
substitution
27) Which has the largest atomic radius?
A. potassium
B. rubidium
C. francium
D. cesium
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28) A sample of helium gas is in a sealed, rigid container. What occurs as the temperature of the
sample is increased?
A.
B.
C.
D.
The mass of the sample decreases.
The number of moles of gas increases.
The volume of each atom decreases.
The frequency of collisions between atoms increases.
29) Which set of compounds below are classified as Arrhenius acids?
A.
B.
C.
D.
HCl and NaOH
HNO3 and NaCl
NH3 and H2CO3
HBr and H2SO4
30) What is the molar mass of Fe(NO3)3?
A.
B.
C.
D.
146 g/mol
194 g/mol
214 g/mol
242 g/mol
31) What is the oxidation number of manganese in KMnO4?
A.
B.
C.
D.
7+
2+
3+
4+
32) What is the number of electrons in an Al3+ ion?
A.
B.
C.
D.
10
13
3
16
33) What is the formula of the compound formed between the potassium ion and the sulfide
ion?
A.
B.
C.
D.
E.
KS
KS2
K2S3
KS3
K2S
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34) How many mL of 0.250 M H2SO4 is required to completely react with 25.0 mL of 1.50 M
NaOH? Below is the balanced equation for the reaction.
H2SO4 (aq) + 2 NaOH (aq) → Na2SO4 (aq) + 2 H2O (l)
A.
B.
C.
D.
150 mL
50 mL
300 mL
75 mL
35) How many grams of calcium bromide, CaBr2, are in 50.0 mL of 0.25 M calcium bromide
solution?
A.
B.
C.
D.
E.
2.5 g
1.5 g
1.3 x 10-2 g
24 g
40 g
36) Compared to the physical and chemical properties of the compound NO2, the compound
N2O has
A.
B.
C.
D.
different physical properties and different chemical properties.
different physical properties and the same chemical properties.
the same physical properties and different chemical properties.
the same physical properties and the same chemical properties.
37) Which substance cannot be broken down by a chemical change?
A.
B.
C.
D.
ammonia
ethanol
carbon dioxide
zirconium
38) Which pair of elements is most likely to form an ionic compound?
A.
B.
C.
D.
E.
barium, bromine
calcium, sodium
oxygen, fluorine
sulfur, fluorine
nitrogen, hydrogen
39) Iron (III) sulfate has the formula
A.
B.
C.
D.
E.
Fe3SO4
Fe2(SO4)3
Fe2(SO3)3
Fe2SO4
Fe2SO3
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40) The graph below represents the uniform heating of a substance from the solid to the gas
phase.
F
Temperature
D
E
B
C
A
Time
Which line segment of the graph represents boiling?
A.
AB
B.
BC
C.
CD
D.
DE