1) When a metal gains an electron, the process is endothermic.
2) The reduction of O2 by sodium hydride produces lye.
3) In radioactive dating, the ratio of carbon-12 to carbon-14 is related to the time of
death of the animal or plant under investigation.
4) There are 6 significant figures in the number 0.003702.
5) The primary component of natural gas is propane.
6) Blackbody radiation is the emission of light from metal surfaces.
7) Temperature is a physical property that determines the direction of heat flow.
8) Adding a nonvolatile solute to a solution decreases the vapor pressure of the solution.
9) Le Ch¢telier’s principle states that if a system at equilibrium is disturbed, the
equilibrium will shift to minimize the disturbance.
10) The compound NH4Cl is a weak acid.
11) Xenon can form compounds with fluorine.
12) Kinetic-molecular theory assumes that attractive and repulsive forces between gas
particles are stronger than those between gas particles and container walls.
13) Work equals force times distance.
14) According to the kinetic-molecular theory, molecules of different gases at the same
temperature always have the same average kinetic energy.
15) In the Lewis structure of ClF, the formal charge on Cl is ________, and the formal
charge on F is ________.
A) -1, -1
B) 0, 0
C) 0, -1
D) +1, -1
E) -1, +1
16) How are the oxygen-containing compounds of xenon made?
A) by direct combination of the elements
B) by reaction of xenon with peroxide
C) by thermal decomposition of the xenon hydroxide
D) by reaction of the corresponding xenon fluoride with water
E) Xenon is inert and does not form compounds with oxygen.
17) The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous
K2Cr2O7 to 500. mL is ________.
A) 0.0879
B) 87.9
C) 0.0218
D) 0.0115
E) 0.870
18) The alkali metal that is naturally radioactive is ________.
A) rubidium
B) cesium
C) lithium
D) francium
E) sodium
19) The balanced reaction between aqueous potassium hydroxide and aqueous acetic
acid is ________.
A) KOH (aq) + HC2H3O2 (aq) → OH– (l) + HC2H3O2
+ (aq) + K (s)
B) KOH (aq) + HC2H3O2 (aq) → H2O (l) + KC2H3O2 (aq)
C) KOH (aq) + HC2H3O2 (aq) → H2C2H3O3 (aq) + K (s)
D) KOH (aq) + HC2H3O2 (aq) → KC2H3O3 (aq) + H2 (g)
E) KOH (aq) + HC2H3O2 (aq) → H2KC2H3O (aq) + O2 (g)
20) Of the following compounds, which is the most stable?
A) XeF6
B) XeOF4
C) XeO3
D) XeO2F2
E) XeF2
21) Of the atoms below, ________ is the most effective in forming € bonds.
A) C
B) P
C) N
D) Si
E) Ge
22) The atomic number of an atom of 80
Br is ________.
A) 115
B) 35
C) 45
D) 73
E) 80
23) At elevated temperatures, molecular hydrogen and molecular bromine react to
partially form hydrogen bromide:
H2 (g) + Br2 (g) 2HBr (g)
A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel
with a volume of
2.00 L. At equilibrium at 700 K, there are 0.546 mol of H2 present. At equilibrium,
there are ________ mol of Br2 present in the reaction vessel.
A) 0.000
B) 0.440
C) 0.546
D) 0.136
E) 0.304
24) What types of intermolecular forces exist between NH3 and H2S?
A) dispersion forces and dipole-dipole forces
B) dispersion forces
C) dispersion forces and hydrogen bonds
D) dispersion forces, hydrogen bonds, and dipole-dipole forces
E) dispersion forces, hydrogen bonds, and ion-dipole forces
25) If an electron has a principal quantum number (n) of 7 and an angular momentum
quantum number (l) of 3, the subshell designation is ________.
A) 7f
B) 7s
C) 7p
D) 3f
E) 3d
26) Of the following transitions in the Bohr hydrogen atom, the ________ transition
results in the emission of the highest-energy photon.
A) n = 6 → n = 4
B) n = 2 → n = 7
C) n = 4 → n = 6
D) n = 1 → n = 4
E) All transitions emit photons of equivalent energy.
27) Given the thermodynamic data in the table below, calculate the equilibrium constant
(at 298 K) for the reaction:
2 SO2 (g) + O2 (g) 2 SO3 (g)
A) 2.40 x 1024
B) 1.06
C) 1.95
D) 3.82 x 1023
E) More data are needed.
28) Which one of the following substances will not have hydrogen bonding as one of its
intermolecular forces?
A)
B)
C)
D)
E)
29) The complete electron configuration of sulfur, element 16, is ________.
A) 1s22s22p63s23p4
B) 1s22s22p103s2
C) 1s42s42p63s2
D) 1s42s42p8
E) 1s62s62p23s2
30) Hydrogen peroxide decomposes to water and oxygen at constant pressure by the
following reaction:
2H2O2 (l) → 2H2O (l) + O2 (g)³ ΔH = -196 kJ
Calculate the value of q (kJ) in this exothermic reaction when 1.50 g of hydrogen
peroxide decomposes at constant pressure?
A) -8.65 kJ
B) -4.32 kJ
C) -0.0578 kJ
D) 3.84 kJ
E) -8.65 x 103 kJ
31) A solution containing 20.0 g of an unknown liquid and 110.0 g water has a freezing
point of -1.32 oC. Given Kf = 1.86 oC/m for water, the molar mass of the unknown
liquid is ________ g/mol.
A) 256
B) 69.0
C) 333
D) 619
E) 78.1
32) The molecular weight of a gas that has a density of 7.10 g/L at 25.0 °C and 1.00 atm
pressure is ________ g/mol.
A) 174
B) 14.6
C) 28.0
D) 5.75 x 10-3
E) 6.85 x 10-2
33) Which isoelectronic series is correctly arranged in order of increasing radius?
A) K+ < Ca2+ < Ar < Cl–
B)Cl– < Ar < K+ < Ca2+
C) Ca2+ < Ar < K+ < Cl–
D) Ca2+ < K+ < Ar < Cl–
E) Ca2+ < K+ < Cl– < Ar
34) In photosynthesis, ________ moles of photons are required to form one mole of
________.
35) In molecular orbital theory, the stability of a covalent body is related to its
________.
36) If the reaction quotient Q for a reaction is greater than the value of the equilibrium
constant K for that reaction at a given temperature, ________ must be converted to
________ for the system to reach equilibrium.
37) A solution of formic acid is 3.0% dissociated at 25.0 oC. What is the original
concentration (in M) of the formic acid solution? The Ka at 25.0 oC for formic acid is
1.8 x 10-4.
38) The addition of an alkyl halide to an aromatic ring compound is called the
________ reaction.
39) The electron configuration of the valence electrons of an atom in its ground state is
ns2np3. This atom is a group ________ element.
40) What halogen, other than astatine, is not usually found in seawater?
41) The fourth most abundant component of dry air is ________.
42) The shape of an orbital is defined by the angular momentum quantum number
which is represented as letter ________.