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Hazen • AP Chemistry
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Period ___ Date ___/___/___
5-7 • Review
PRACTICE TEST
1.
On the basis of the solubility rules, which of the following is insoluble?
a) K2O
d) (NH4)2SO4
b) Na2CO3
e) Ba(C2H3O2)2
c) PbS
2.
In a double replacement reaction, formation of which of the following does not necessarily lead to a
chemical change?
a) HC2H3O2
d) H2S
b) AgCl
c) CO2
e) NaCl
3.
Reaction of an acid with a carbonate (such as CaCO3) always results in the formation of
a) O2
d) O3
b) C(diamond)
e) CO2
c) CH4
4.
Which of the following is incorrect?
a) all salts containing NH4+ are soluble.
b) all salts containing NO3– are soluble.
c) all fluorides are soluble.
d) all sulfates (except those of Ca2+, Sr2+, Ba2+, and Pb2+) are soluble.
e) most hydroxides are insoluble, except those of Ca2+, Sr2+, Ba2+, the alkali metals and NH4+.
5.
One of the gases shown below is NOT usually formed in a double replacement reaction. Which one?
a) N2
d) NH3
b) CO2
e) H2S
c) SO2
6.
Write the balanced molecular equation for the reaction of washing soda, Na2CO3 and vinegar,
HC2H3O2.
7.
The net ionic equation for the above reaction is:
8.
How many moles of H+ are associated with the acid, H2SO3, during neutralization?
a) 0
9.
b) 1
c) 2
d) 3
How many moles Al2O3 are needed to neutralize 1 mole of HCl?
a) 1/3
d) 6
b) 2/3
e) 12
c) 2
f)
1/
6
10. Write the net reaction that will occur when solid ammonium carbonate is added to a solution of
hydrosulfuric acid.
11. When H2SO4 and Ba(OH)2 are reacted in a double replacement reaction, one of the products of the
reaction is…
a) H2
d) BaH2
b) H2O
e) SO2
c) BaS
12. In the double replacement reaction between the weak acid, HC2H3O2 and strong base, NaOH, which
ion(s) are spectator ions?
a) Na+, C2H3O2–
d) H+, C2H3O2–
b) Na+, OH–
c) OH– only
e) Na+ only
13. Which of the following is a base?
a) KOH
d) CH3OH
b) C2H5OH
e) CO2
c) Br–
14. Which of the following is a strong acid?
a) H2CO3
d) HClO3
b) HF
e) HNO3
c) H3PO4
15. Which of the following is an acid in aqueous solutions?
a) H2CO3
d) H2O
b) Al2O3
e) BaO
c) CH4
16. SO2 turns into which acid in solution?
a) HNO3
d) H2S
b) H2SO3
e) HNO2
c) H2SO4
17. What is the oxidation number of C in CO32–?
a) +6
b) +4
c) +2
d) +1
e) –1
18. What is the oxidation number of Br in KBrO4?
a) +1
b) –1
c) +5
d) +7
e) +8
19. For each change below, label the change of the underlined element as Oxidation, Reduction, or Neither
___ Cu2+  Cu
___ CH4  CO2
___ H2O2  H2O
___ CO2  H2CO3
20. How many milliliters of 0.123 M NaOH solution contain 25.0 g of NaOH (molar mass = 40.00 g/mol)?
a) 5.08 mL
d) 625 mL
b) 50.8 mL
e) 5080 mL
c) 508 mL
21. If you need 1.00 L of 0.125 M H2SO4, how would you prepare this solution?
a) Add 950. mL of water to 50.0 mL of 3.00 M H2SO4.
b) Add 500. mL of water to 500. mL of 0.500 M H2SO4.
c) Add 750 mL of water to 250 mL of 0.375 M H2SO4.
d) Dilute 36.0 mL of 1.25 M H2SO4 to a volume of 1.00 L.
e) Dilute 20.8 mL of 6.00 M H2SO4 to a volume of 1.00 L.
22. What is the ion concentration in a 0.12 M solution of BaCl2?
a) [Ba2+] = 0.12 M and [Cl] = 0.12 M.
b) [Ba2+] = 0.12 M and [Cl] = 0.060 M.
c) [Ba2+] = 0.12 M and [Cl] = 0.24 M.
d) [Ba2+] = 0.060 M and [Cl] = 0.060 M.
e) [Ba+] = 0.12 M and [Cl2] = 0.12 M.
23. What is the molarity of the solution that results when 60.0 g NaOH is added to enough water to make
500. mL solution?
a) 1.33 M
d) 8.0 M
b) 12.0 M
e) 1.50 M
c) 3.00 M
24. What is the molarity of the solution that results when 45.0 g HCl is dissolved in enough water to make
250. mL solution?
a) 4.94 M
d) 1.80 M
b) 4.50 M
e) 1.46 M
c) 3.24 M
25. What is the concentration of Cl– ion in 0.60 M AlCl3 solution?
a) 1.8 M
b) 0.60 M
d) 0.30 M
e) 0.10 M
c) 0.20 M
26. How many grams of Na2CO3 (molar mass = 106.0 g/mol) are required for complete reaction with 25.0
mL of 0.155 M HNO3?
Na2CO3 + 2HNO3  2NaNO3 + CO2 + H2O
a) 0.122 g
b) 0.205 g
c) 0.410 g
d) 20.5 g
e) 205 g
27. What volume of 0.150 M NaOH is needed to react completely with 3.45 g iodine according to the
equation:
3 I2 + 6 NaOH  5 NaI + NaIO3 + 3 H2O
a) 181 mL
b) 45.3 mL
c) 4.08 mL
d) 2.04 mL
e) 1.02 mL
28. What is the concentration of an NaOH solution if it takes 16.25 mL of a 0.100 M HCl solution to titrate
25.00 mL of the NaOH solution?
a) 0.0165 M
d) 0.100 M
b) 0.151 M
e) 0.413 M
c) 0.0650 M
29. A 4.00 M solution of H3PO4 will contain ___g of H3PO4 in 0.250 L of solution.
a) 196 g
b) 98.0 g
c) 49.0 g
d) 24.0 g
e) 12.0 g
30. How many joules are equivalent to 37.7 cal?
a) 9.01 J
c) 1.51 J
b) 4.184 J
d) 158 J
31. The quantity of heat that is needed to raise the temperature of a sample of a substance 1.00 degree is
called its
a) heat capacity
b) specific heat
c) enthalpy
d) kinetic energy
32. Equal masses of two substances, A & B, each absorb 25 Joules of energy. If the temperature of A
increases by 4 degrees and the temperature of B increases by 8 degrees, one can say that
a) the specific heat of A is double that of B.
b) the specific heat of B is double that of A.
c) the specific heat of B is negative.
d) the specific heat of B is triple that of A.
33. If 25 J are required to change the temperature of 5.0 g of substance A by 2.0C, what is the specific heat
of substance A?
a) 250 J/gC
c) 10. J/gC
b) 63 J/gC
d) 2.5 J/gC
34. How much energy is required to change the temperature of 2.00 g aluminum from 20.0C to 25.0C?
The specific heat of aluminum is 0.902 J/gC.
a) 2.3 J
b) 9.0 J
c) 0.36 J
d) 0.090 J
35. Consider the thermal energy transfer during a chemical process. When heat is transferred to the system,
the process is said to be _______ and the sign of H is ________.
a) exothermic, positive
b) endothermic, negative
c) exothermic, negative
d) endothermic, positive
36. What is the E for a system which has the following two steps:
Step 1: The system absorbs 60 J of heat
while 40 J of work are performed on it.
Step 2: The system releases 30 J of heat
while doing 70 J of work.
a) 100 J
c) 30 J
b) 90 J
d) zero
37. When two solutions react the container “feels hot.” Thus,
a) the reaction is endothermic.
b) the reaction is exothermic.
c) the energy of the universe is increased.
d) the energy of both the system and the surroundings is decreased.
38. The equation for the standard enthalpy of formation of N2O3 is
a) N2O(g) + O2(g)  N2O3(g)
b) N2O5(g)  N2O3(g) + O2(g)
c) NO(g) + NO2(g)  N2O3(g)
d) N2(g) + 3/2 O2(g)  N2O3(g)
39. For the general reaction
2 A + B2  2 AB,
H is +50.0 kJ.
We can conclude that
a) the reaction is endothermic.
b) the surroundings absorb energy.
c) the standard enthalpy of formation of AB is -50.0 kJ.
d) the molecule AB contains less energy than A or B2.
40.
Calculate the enthalpy of combustion of C3H6:
C3H6(g) + 9/2O2(g)  3CO2 + 3H2O
using the following data:
3C(s) + 3H2(g)  C3H6(g)
H= 53.3 kJ
C(s) + O2(g)  CO2(g)
H=-394 kJ
H2(g) + 1/2O2(g)  H2O(l)
H=-286 kJ
a) -1517 kJ
c) -626 kJ
b) 1304 kJ
d) -2093 kJ
41. Which one of the following would have an enthalpy of formation value (Hf) of zero?
a) H2O(g)
c) H2O(l)
b) O(g)
d) O2(g)
42. Calculate the heat of vaporization of titanium (IV) chloride: TiCl4(l)  TiCl4(g)
using the following enthalpies of reaction:
Ti(s) + 2Cl2(g)  TiCl4(l) H=-804.2 kJ
TiCl4(g)  2Cl2(g) + Ti(s) H= 763.2 kJ
a) -1567 kJ
c) 1165 kJ
b) -783.7 kJ
d) 41 kJ
43. Calculate the enthalpy of reaction for:
D+FG+M
using the following equations and data:
G+CA+B
H = +277 kJ
C+FA
DB+M
a) -132 kJ
b) -422 kJ
H = +303 kJ
H = -158 kJ
c) +422 kJ
d) +132 kJ
44. Calculate the standard enthalpy of the reaction for the process
3NO(g)  N2O(g) + NO2(g)
using the standard enthalpies of formation (in kJ/mol): NO = 90; N2O = 82.1; NO2 = 34.0
a) -153.9 kJ
b) 206 kJ
c) -26.1 kJ
d) 386 kJ
45. The standard molar enthalpy of combustion is
-1277.3 kJ for the combustion of ethanol.
C2H5OH(l) + 3O2(g)  2CO2(g) + 3H2O(g)
Calculate the standard molar enthalpy of formation for ethanol based on the following standard
enthalpies of formation:
Hf CO2 = -393.5 kJ/mol
Hf H2O = -241.8 kJ/mol
a) -642.7 kJ/mol
c) 235.1 kJ/mol
b) -235.1 kJ/mol
d) 642.7 kJ/mol
46. Calculate the amount of heat needed to change 25.0 g ice at 0C to water at 0C.
The heat of fusion of H2O = 333 J/g;
a) 56.5 kJ
c) 7.06 kJ
b) 8.33 kJ
d) 463 kJ
Questions 47-49: (1/2 point each)
The following data was collected in an experiment similar to the Specific Heat experiment performed in
class. Fill in the missing values. (Assume the calorimeter has a calorimeter constant of 0 J/C)
Data & Calculations
mass of glass beads
4.88 g
mass of water
10.14 g
initial temperature of water
19.2 C
initial temperature of beads
89.2 C
final temperature of mixture
24.8 C
18.
temp change of water (C)
18.
temp change of hot beads (C)
19.
change in energy of water, qwater (J)
change in energy of calorimeter (J)
19.
change in energy of beads, qbeads (J)
20.
specific heat of beads (J·g-1·C-1)
accepted value of specific heat
20.
Glass
Beads
% error
0J
.833
A = 2.18 x 10-18 J
h = 6.626 x 10-34 J·s
R = 1.097 x 107 m–1
c = 3.00 x 108 m·s–1
mass of an electron = 9.11 x 10-31 kg
50. What wavelength corresponds to a frequency of
8.22 x 109 Hz?
a) 0.307 m
d) 0.110 m
b) 0.0365 m
e) 27.4 m
c) 0.122 m
51. A radio station transmits at 110 MHz (110 x
106 Hz). What wavelength is this radio wave?
a) 3.65 x 10–5 m
c) 3.81 x 10–5 m
b) 3.30 m
d) 2.73 m
52. Which one of the following is NOT a proper
unit for frequency?
a) Hz
c) m·s–1
b) s–1
d)
56. What is the de Broglie wavelength of an
electron moving at 80.0% the speed of light.
a) 3.03 x 10–12 m
c) 3.30 x 1011 m
b) 2.42 x 10–12 m
d) 1.59 x 10–25 m
57. What resultant is expected from the
interference of the two waves shown below?
1
sec
53. Calculate the wavelength of the fourth line in
the Balmer series (the visible series) of the
hydrogen spectrum.
a) 0.12334 m
d) 4.1029 x 10–7 m
b) 24.373 m
e) 36.559 m
c) 2.7353 x 10–7 m
54. What is the relationship between the energy of
a photon of light and its frequency?
1
a) E = 
d) E =
h
h

b) E =
e) E = h

c) E = h
55. What is the energy needed to raise an electron
in the hydrogen atom from the second energy
level to the third energy level?
a) 1.52 x 104 J
d) 4.48 x 10–19 J
b) 3.63 x 10–19 J
e) 3.03 x 10–19 J
c) 2.18 x 10–19 J
a)
c)
b)
d)
58. Which quantum number determines the
subshell occupied by an electron (s, p, d, f,
etc.)?
n
b) l
a)
c)
d)
ml
ms
59. What position on the standing wave shown
below corresponds to a crest?
64. Which of the following sets of quantum
numbers is possible for a 3d electron?
n = 3, l = 3, ml = –2, ms = +12
1
b) n = 2, l = 1, ml = +1, ms = – 2
1
c) n = 3, l = 1, ml = 0, ms = – 2
1
d) n = 3, l = 2, ml = –2, ms = +2
1
e) n = 4, l = 1, ml = +1, ms = +2
a)
a) A
b) B
c) C
d) D
e) E
60. How many orbitals make up the 4d subshell?
a) 0
b) 1
c) 3
d) 5
e) 7
61. The value of l that is related to the following
orbital is:
a) 0
b) 1
c) 2
d) 3
e) 4
62. The correct electron configuration for nitrogen
is
a)
b)
c)
d)
e)
1s2 2s2 2p6 3s2 3p2
1s2 2s2 2p6 2d4
1s2 2s2 2p3
1s2 2s2 3s2 4s1
1s2 1p5
63. The electron configuration of the indicated
atom in the ground state is correctly written for
which atom?
a) Ga
[Ar] 3d12 4s2
b) Ni
c) Ni
d) Cu
[Ar] 3d10
[Ar] 3s2 3p8
[Ar] 3d10 4s1
65. In what section of the periodic table is the 4f
subshell being filled?
a)
b)
c)
d)
e)
period 4
transition elements Y to Cd
noble gases
group IA
lanthanides
66. Which one of the following elements has 3
electrons in a p subshell?
a) Sb
b) Na
c) Sc
d) V
e) Nd
67. Which of the following distributions of
electrons is correct for three electrons in psubshell?
a)



b)


c)


d)


e)



68. Which of the following particles would be most
paramagnetic?
a) P
b) Ga
c) Br
d) Cle) Na+
69. Which of the following correctly represents the
ionization of an atom?
a)
b)
c)
d)
Cl(g) + e–  Cl–(g)
Na(g)  Na+(g) + e–
Na(s) – e–  Na+(g)
Cl2(g)  2 Cl(g)
75. Draw the orbital diagram for a neutral Ag
atom:
5s
4s
3s
70. Which of the following is likely to have the
largest atomic radius?
a) H
b) Mn
c) Cl
d) Rb
e) Ag
2s
71. Which one of the following isoelectronic
1s
species has the smallest radius?
a) Mg2+
d) F –
b) Na+
e) O2–
c) Ne
NOTE: explain your reasoning on the last page.
72. Which of the following has the greatest
ionization energy?
a) K
b) Ca
c) Fe
d) Ga
e) Br
73. Which of the following has the lowest
ionization energy?
a) Li
b) Na
c) K
d) Rb
e) Cs
74. The successive ionization energies for one of
the period three elements is listed below.
Which element is referred to?
E1
577.4 kJ/mol
E2
1,816 kJ/mol
E3
2,744 kJ/mol
E4
11,580 kJ/mol
E5
15,030 kJ/mol
a) Na
b) Mg
c) Al
d) Si
e) P
NOTE: explain your reasoning on the last
page.
Write the electron configuration for silver:
76. Long form:
77. Short form:
78. Explain your answer to question 22.
Which one of the following isoelectronic
species has the smallest radius?
a) Mg2+
b) Na+
c) Ne
d) F –
e) O2–
79. Explain your answer to question 25.
The successive ionization energies for one of the period three elements is listed below. Which element is
referred to?
E1
577.4 kJ/mol
a) Na
b) Mg
c) Al
d) Si
E2
1,816 kJ/mol
E3
2,744 kJ/mol
E4
11,580 kJ/mol
E5
15,030 kJ/mol
e) P
1.