59. Which of the following concerning molecular geometry and dipole moments is/are correct?
1.
Only molecules with polar bonds may have a permanent dipole moment.
2.
All molecules with polar bonds have a permanent dipole moment.
3.
All square planar molecules are nonpolar.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 3
E)
1, 2, and 3
60. Which of the following molecules has a permanent dipole moment?
A)
SF6
B)
CCl4
C)
NF3
D)
SiCl4
E)
BF3
61. Which of the following molecules does not have a permanent dipole moment?
A)
sulfur tetrafluoride, SF4
B)
iodine trichloride, ICl3
C)
nitrogen trifluoride, NF3
D)
phosphorus pentafluoride, PF5
E)
sulfur dioxide, SO2
62. Which of the following molecules has a dipole moment?
A)
PF5
B)
FOOF
C)
HCCH
D)
F2CCF2
E)
SF6
63. Which of the following molecules has a dipole moment?
A)
SO2
B)
CS2
C)
ClCCCCCl
D)
CCl4
E)
HCCH
64. Which of the following compounds is nonpolar?
A)
H2S
B)
XeF2
C)
SO2
D)
N2O
E)
HCl
65. Which of the following molecules is polar?
A)
SF6
B)
CCl4
C)
BF3
D)
NO2
E)
CO2
66. Which of the following statements best describes N2O?
A)
The molecular geometry is bent and the molecule is nonpolar.
B)
The molecular geometry is linear and the molecule is nonpolar.
C)
The molecular geometry is linear and the molecule is polar.
D)
The molecular geometry is trigonal planar and the molecule is nonpolar.
E)
The molecular geometry is bent and the molecule is polar.
Test Bank General Chemistry, 10th edition 19
67. Which of the following molecules is nonpolar?
A)
SF4
B)
PF5
C)
ClF3
D)
PF3
E)
CH2F2
68. Which one of the following statements provides the best evidence that all the carbon
compounds listed below have tetrahedral molecular geometries instead of square planar
molecular geometries?
A)
Only one CH4 compound is known and it is nonpolar.
B)
Only one CH3F compound is known and it is polar.
C)
Only one CH2F2 compound is known and it is polar.
D)
Only one CF4 compound is known and it is nonpolar.
E)
Only one CHF3 compound is known and it is polar.
69. When an atom in a molecule or ion is described as sp3d2 hybridized, its molecular geometry
is
A)
octahedral.
B)
trigonal bipyramidal.
C)
linear.
D)
tetrahedral.
E)
trigonal planar.
70. How many sigma and pi bonds are in the molecule pictured below?
A)
thirteen sigma bonds and one pi bond
B)
eleven sigma bonds and two pi bonds
C)
thirteen sigma bonds and two pi bonds
D)
eleven sigma bonds and five pi bonds
E)
five sigma bonds and eleven pi bonds
71. What hybrid orbitals of sulfur are involved in the bonding in sulfur trioxide?
A)
sp2
B)
sp2d
C)
sp3
D)
sp3d2
E)
sp
72. Which of the following statements is incorrect regarding the water molecule?
A)
There are two lone pairs and two bonding pairs on the central atom.
B)
The molecule is polar.
C)
The hybridization of oxygen is sp3.
D)
The hybridization of hydrogen is sp.
E)
The molecular geometry is bent.
73. What is the hybridization of Se in SeF6?
A)
sp3d
B)
sp3d2
C)
sp2
D)
sp
E)
sp3
Test Bank General Chemistry, 10th edition 21
74. What is the hybridization of Br in BrF3?
A)
sp3
B)
sp
C)
sp3d2
D)
sp2
E)
sp3d
75. What is the hybridization of I in IF4–?
A)
sp2
B)
sp
C)
sp3d
D)
sp3d2
E)
sp3
76. According to valence-bond theory, what is the hybridization scheme of the sulfur atom in
SF4?
A)
B)
C)
Test Bank General Chemistry, 10th edition 22
D)
E)
77. A bond is the result of the
A)
overlap of two s orbitals.
B)
overlap of two p orbitals along their axes.
C)
sideways overlap of two parallel p orbitals.
D)
overlap of an s orbital and a p orbital.
E)
sideways overlap of two s orbitals.
78. Which of the following statements is true?
A)
A bond is twice as strong as a single bond.
B)
A bond results from the sideways overlap of hybridized orbitals.
C)
A double bond consists of a bond and a bond.
D)
A bond has cylindrical symmetry about the bonding axis.
E)
A bond is twice as strong as a bond.
79. Which of the labeled carbons (C1-C4) is/are sp3-hybridized?
Test Bank General Chemistry, 10th edition 23
A)
carbon two and four
B)
carbon three
C)
carbon one
D)
carbon two
E)
carbon one and three
80. What is the hybridization of the nitrogen atom in the nitrite ion?
A)
sp3d
B)
sp3
C)
s
D)
sp
E)
sp2
81. According to valence-bond theory, the bonding in ketene, H2CCO, is best described as
A)
five bonds.
B)
three bonds and two bonds.
C)
four bonds and two bonds.
D)
four bonds and one bond.
E)
five bonds.
82. Which of the following concerning and bonds is/are correct?
1.
Sigma bonds may only be formed from unhybridized orbitals.
2.
Pi bonds are formed from unhybridized p orbitals.
3.
A pi bond has an electron distribution above and below the bond axis.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
2 and 3
83. Which of the following concerning and bonds is/are correct?
1.
A sigma bond may be formed from the sideways overlap of two parallel p
orbitals.
2.
No more than two pi bonds are possible between adjacent carbon atoms.
3.
The considerable energy required to rotate pi bonded atoms is the primary
reason for geometrical isomerism in some pi bonded molecules.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
2 and 3
84. Which molecule or ion does not contain two bonds?
A)
HCCH
B)
H2CCCH2
C)
NO–
D)
CS2
E)
SCN–
85. If four orbitals on one atom overlap four orbitals on a second atom, how many molecular
orbitals will form?
A)
4
B)
16
C)
1
D)
8
E)
none of these
86. Which of the following statements is/are true?
1.
Electrons are never found in an antibonding molecular orbital.
2.
Antibonding molecular orbitals have electron density mainly outside the space
between the two nuclei.
3.
All antibonding molecular orbitals are higher in energy than the atomic
orbitals of which they are composed.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
2 and 3
87. The nitrosyl ion, NO+, has ten bonding electrons and four antibonding electrons. Therefore,
it has a bond order of
A)
1.
B)
5/2.
C)
7.
D)
2.
E)
3.
88. Which of the following species has(have) a bond order of 2?
1. NO–
2. O2
3. O2–
A)
1 only
B)
3 only
C)
2 only
D)
1 and 3
E)
1 and 2
Test Bank General Chemistry, 10th edition 26
89. Which of the following species has a bond order of 2.5?
A)
N2
B)
NO+
C)
CO
D)
O2+
E)
NO–
90. Which molecule or ion has a bond order of 2.5?
A)
O2
B)
O2+
C)
NO–
D)
O22–
E)
O2–
91. Which of the following species has(have) a bond order of 1?
1. HF
2. O22−
3. O22+
A)
1 only
B)
3 only
C)
1 and 2
D)
2 and 3
E)
2 only
92. Given the molecular orbital diagram for dilithium (Li2) below, what would be the bond
order of Li2+?
Test Bank General Chemistry, 10th edition 27
A)
B)
C)
1
D)
0
E)
2
93. Which of the following statements is not correct?
A)
Hybrid orbitals are made by the combination of atomic orbitals on a given atom.
B)
In both valence bond theory and molecular orbital theory bonding result from the
overlap of occupied atomic orbitals.
C)
Valence bond theory does not account for the experimentally observed
paramagnetism of molecules like O2.
D)
Pi bonds may be formed from s or p orbital overlap.
E)
In molecular orbital theory a molecular orbital may encompass more than two
atoms.
94. Given the molecular orbital diagram for dinitrogen (N2) excluding the K shells below, which
of the following molecules or ions is expected to be diamagnetic?
A)
C22–
B)
O2
C)
B2
D)
O2–
E)
O2+
95. Which molecule or ion has the highest bond order?
A)
F2–
B)
O2
C)
O22–
D)
N2
E)
F2
96. Given the molecular orbital diagram for dinitrogen (N2) excluding the K shells below and
assuming all species have a similar ordering of their MO’s, which of the following would be
expected to be diamagnetic?
A)
O2
B)
F2−
C)
O2−
D)
B2
E)
Li2+
Test Bank General Chemistry, 10th edition 29
97. Consider the following series of molecular ions and molecules: F2+, F22+, F2, and F2–. Which
will have the shortest bond length between the fluorine atoms? Assume the homonuclear
molecular orbital diagram provided below for nitrogen (excluding the K shells) still applies
to these species.
A)
F2+
B)
The bond lengths are all equivalent.
C)
F22+
D)
F2
E)
F2–
98. The configuration (2s)2(2s*)2(2py)1(2px)1 is the molecular orbital description for the
ground state of
A)
C2.
B)
B2.
C)
Be2.
D)
Li2+.
E)
B22–.
99. Which molecule or ion has the shortest bond distance?
A)
NO+
B)
CO+
C)
NO
D)
NO–
E)
CO–
Test Bank General Chemistry, 10th edition 30
100. In the molecular orbital description of CO,
A)
six molecular orbitals contain electrons.
B)
there are two unpaired electrons.
C)
the bond order is 3.
D)
the highest-energy electrons occupy antibonding orbitals.
E)
All of the above are false.
101. Which of the following electron distributions among the molecular orbitals best describes
the NO molecule?
2s
2s*
2py=2px
2pz
2py*=2px*
2pz*
A)
2 2 4 1 3 0
B)
2 2 4 2 4 1
C)
2 2 4 2 1 0
D)
2 2 4 2 2 0
E)
2 2 4 2 4 2
102. Which of the following statements about the molecule O2 is false?
A)
Its bond order is 2.
B)
The total number of electrons is 12.
C)
It is paramagnetic.
D)
It has two pi bonds.
E)
It has one sigma bond.
103. Which molecule or ion is paramagnetic?
A)
NO2+
B)
OCN–
C)
NO2–
D)
NO
E)
SO3
104. Which of the following statements concerning ozone is incorrect?
A)
It is generated by passing an electrical discharge through oxygen.
B)
It has a partial double-bond character.
C)
It is a nonpolar molecule.
D)
It is an important absorber of ultraviolet radiation in the stratosphere.
E)
It has a bond angle similar to that predicted for sp2 hybridization.
105. Which of these statements about benzene is true?
A)
Benzene is an example of a molecule that displays ionic bonding.
B)
Benzene contains only bonds between C atoms.
C)
All carbon atoms in benzene are sp3 hybridized.
D)
The bond order of each C—C bond in benzene is 1.5.
E)
All of these statements are false.
106. The following statements concern molecules that require resonance. Which is true?
A)
The benzene molecule is best described by the MO theory.
B)
The sigma bonding is clearly delocalized.
C)
Both the sigma bonding and the pi bonding are delocalized.
D)
The benzene molecule is best described by the localized electron model.
E)
The pi bonding is clearly delocalized.