Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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Which
of the following are resonance structures for nitrite ion,
NO2-?
a. | 1 and
2 | b. | 2 and
4 | c. | 1,2 and
3 | d. | 2 and
3 | e. | 1, 2 and
4 | | |
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2.
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Which
of the following are resonance structures for formate ion,
HCO2-?
a. | 1 and
2 | b. | 2 and
3 | c. | 1 and
3 | d. | 1 and
4 | e. | 1, 2 and
4 | | |
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3.
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The
central atom in SF4 is surrounded by a. | 4 single bonds, no double bonds, and no lone pairs of
electrons. | b. | 4 single bonds, no double bonds, and 1 lone pairs of
electrons. | c. | 3 single bonds, 1 double bond, and 1 lone pair of
electrons. | d. | 2 single bonds, 2 double bonds, and no lone pairs of
electrons. | e. | no single bonds, 4 double bonds, and 2 lone pairs of
electrons. | | |
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4.
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The
central atom in BrF5 is surrounded by a. | 5 single bonds, no double bonds, and no lone pairs of
electrons. | b. | 5 single bonds, no double bonds, and 1 lone pair of
electrons. | c. | 4 single bonds, 1 double bond, and no lone pairs of
electrons. | d. | 3 single bonds, 2 double bonds, and no lone pairs of
electrons. | e. | 2 single bonds, 2 double bonds, and 2 lone pairs of
electrons. | | |
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5.
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Pure
covalent bonds, ones where the bonding electrons are shared equally between two atoms, only exist
for a. | period 2
nonmetals. | b. | group 4A nonmetals. | c. | metals. | d. | bonds between two identical atoms. | e. | ionic
compounds. | | |
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6.
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Electronegativity is a measure of a. | the charge on an electron. | b. | a molecule's
polarity. | c. | the charge on an atom. | d. | the number of
extra electrons on an anion. | e. | an atom's ability to attract electrons to
itself. | | |
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7.
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Predict which of the following compounds will have the bond that is most
polar.
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8.
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When
heated, azomethane decomposes into nitrogen gas and methane gas.
CH3N=NCH3(g) ®
N2(g) + C2H6(g)
Bond | Bond Enthalpy (kJ/mol) | |
Bond | Bond Enthalpy
(kJ/mol) | C-H | 413 | | N-N | 163 | C-N | 305 | | N=N | 418 | C-C | 346 | | NºN | 945 | | | | | |
Using average
bond enthalpies, calculate the enthalpy of reaction. a. | -609
kJ/mol | b. | -583 kJ/mol | c. | -462
kJ/mol | d. | -263 kJ/mol | e. | -197
kJ/mol | | |
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9.
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Use
VSEPR theory to predict the electron pair geometry and the molecular geometry of
SO2. a. | e-
pair geometry = trigonal planar, molecular geometry = bent | b. | e-
pair geometry = trigonal planar, molecular geometry = linear | c. | e-
pair geometry = tetrahedral, molecular geometry = bent | d. | e-
pair geometry = tetrahedral, molecular geometry = trigonal planar | e. | e-
pair geometry = tetrahedral, molecular geometry = linear | | |
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10.
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Use
VSEPR theory to predict the molecular geometry HCN. a. | bent | b. | linear | c. | trigonal
planar | d. | tetrahedral | e. | octahedral | | |
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11.
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Use
VSEPR theory to predict the molecular geometry of BCl3. a. | bent | b. | trigonal pyramidal | c. | trigonal
planar | d. | tetrahedral | e. | t-shaped | | |
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12.
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What
are the bond angles in SiH4? a. | 90° | b. | 109° | c. | 120° | d. | 180° | e. | 90° and 109° | | |
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13.
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Which
of the following molecules have a dipole moment: CHCl3, NH2Br, NH3,
and BH3? a. | NH3 and BH3 | b. | CHCl3
only | c. | CHCl3, NH2Br, and NH3 | d. | CHCl3
and NH2Br | e. | CHCl3, NH2Br, NH3, and
BH3 | | |
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14.
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How
many sigma (s) bonds and pi
(p) bonds are in acetone?
a. | eight
s and one
p | b. | six s and one p | c. | nine s and one p | d. | one s and nine p | e. | one s and eight p | | |
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15.
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In
order to form a set of sp3d hybrid orbitals, how many pure atomic orbitals
must be mixed? a. | one s,
one p, and one d | b. | one s, three p, and one
d | c. | two s, one p, and two
d | d. | two s, six p, and two
d | e. | none of the above | | |
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16.
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What
is the maximum number of hybridized orbitals that can be formed by xenon?
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17.
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In
which of the following molecules or ions does the central atom have sp3
hybridization: SO42-, XeF4, ICl4-, and
NH3? a. | SO42- and NH3 | b. | SO42- and ICl4- | c. | XeF4
and NH3 | d. | ICl4- and
NH3 | e. | XeF4, ICl4-, and
NH3 | | |
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18.
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What
is the hybridization of each oxygen atom in O2? a. | sp | b. | sp2 | c. | sp3 | d. | sp3d | e. | sp3d2 | | |
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19.
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What
is the hybridization of the sulfur atom in sulfate ion, SO42-? a. | sp | b. | sp2 | c. | sp3 | d. | sp3d | e. | sp3d2 | | |
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20.
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What
is the molecular geometry around an atom that is sp3 hybridized, has three sigma
bonds, no pi bonds, and one lone pair? a. | bent | b. | linear | c. | trigonal
pyramidal | d. | trigonal planar | e. | tetrahedral | | |
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