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Chemistry: A Molecular Approach, 2e (Tro)
Chapter 10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular
Orbital Theory
Multiple Choice Questions
1) Give the approximate bond angle for a molecule with an octahedral shape.
A) 109.5°
B) 180°
C) 120°
D) 105°
E) 90°
2) Determine the electron geometry (eg) and molecular geometry(mg) of BCl3.
A) eg=trigonal planar, mg=trigonal planar
B) eg=tetrahedral, mg=trigonal planar
C) eg=tetrahedral, mg=trigonal pyramidal
D) eg=trigonal planar, mg=bent
E) eg=trigonal bipyramidal, mg= trigonal bipyramidal
3) Determine the electron geometry (eg) and molecular geometry (mg) of CO32⁻.
A) eg=tetrahedral, mg=tetrahedral
B) eg=tetrahedral, mg=trigonal pyramidal
C) eg=trigonal planar, mg=bent
D) eg=trigonal planar, mg=trigonal planar
E) eg=tetrahedral, mg=trigonal planar
4) Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1.
A) eg=tetrahedral, mg=tetrahedral
B) eg=tetrahedral, mg=trigonal pyramidal
C) eg=trigonal planar, mg=bent
D) eg=trigonal planar, mg=trigonal planar
E) eg=tetrahedral, mg=trigonal planar
5) Determine the electron geometry (eg) and molecular geometry (mg) of SiF4.
A) eg=tetrahedral, mg=trigonal pyramidal
B) eg=octahedral, mg=square planar
C) eg=trigonal bipyramidal, mg=trigonal pyramidal
D) eg=tetrahedral, mg=bent
E) eg=tetrahedral, mg=tetrahedral
6) Determine the electron geometry (eg) and molecular geometry (mg) of PF5.
A) eg=trigonal bipyramidal, mg=trigonal bipyramidal
B) eg=octahedral, mg=octahedral
C) eg=trigonal bipyramidal, mg=tetrahedral
D) eg=tetrahedral, mg=trigonal pyramidal
E) eg=trigonal planar, mg=octahedral
7) Determine the electron geometry (eg) and molecular geometry (mg) of CO2.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, mg=trigonal planar
C) eg=trigonal planar, mg=bent
D) eg=linear, mg=linear
E) eg=trigonal planar, mg=trigonal planar
8) The bond angle in NH3 is
A) 107°
B) 104.5°
C) 120°
D) 109.5°
E) 95°
9) The bond angle in H2O is
A) 107°
B) 104.5°
C) 120°
D) 109.5°
E) 95°
10) Determine the electron geometry (eg) and molecular geometry (mg) of NCl3.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, mg=trigonal planar
C) eg=trigonal planar, mg=bent
D) eg=linear, mg=linear
E) eg=tetrahedral, mg=trigonal pyramidal
11) Determine the electron geometry (eg) and molecular geometry (mg) of ICl3.
A) eg=trigonal planar, mg=trigonal planar
B) eg=trigonal bipyramidal, mg= T-shape
C) eg=trigonal planar, mg=bent
D) eg=trigonal bipyramidal, mg=see-saw
E) eg=tetrahedral, mg=trigonal pyramidal
12) Determine the electron geometry (eg) and molecular geometry (mg) of ICl2⁻.
A) eg=tetrahedral, mg=bent
B) eg=tetrahedral, mg=trigonal pyramidal
C) eg=trigonal bipyramidal, mg=linear
D) eg=trigonal bipyramidal, mg=trigonal planar
E) eg=octahedral, mg=linear
13) Determine the electron geometry (eg) and molecular geometry (mg) of XeF2.
A) eg=trigonal bipyramidal, mg=bent
B) eg=linear, mg=linear
C) eg=tetrahedral, mg=linear
D) eg=trigonal bipyramidal, mg=linear
E) eg=tetrahedral, mg=bent
14) Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, eg=linear
C) eg=tetrahedral, mg=bent
D) eg=trigonal bipyramidal, mg=tetrahedral
E) eg=octahedral, mg=square planar
15) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined atom
CH3OCH3.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, eg=linear
C) eg=tetrahedral, mg=bent
D) eg=trigonal bipyramidal, mg=tetrahedral
E) eg=octahedral, mg=square planar
16) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined atom
CH3OCH3.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, eg=linear
C) eg=tetrahedral, mg=bent
D) eg=trigonal bipyramidal, mg=tetrahedral
E) eg=octahedral, mg=square planar
17) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined atom H2CO.
A) eg=tetrahedral, mg=tetrahedral
B) eg=trigonal planar, eg=trigonal planar
C) eg=tetrahedral, mg=bent
D) eg=trigonal bipyramidal, mg=tetrahedral
E) eg=octahedral, mg=square planar
18) Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.
A) C1 = tetrahedral, C2 = linear
B) C1 = trigonal planar, C2= bent
C) C1 = bent, C2 = trigonal planar
D) C1 = trigonal planar, C2 = tetrahedral
E) C1 = trigonal pyramidal, C2 = see-saw
19) Consider the molecule below. Determine the molecular geometry at each of the 3 labeled atoms.
A) 1=trigonal planar, 2=tetrahedral, 3=trigonal pyramidal
B) 1=tetrahedral, 2=tetrahedral, 3=tetrahedral
C) 1=trigonal planar, 2=tetrahedral, 3=tetrahedral
D) 1=tetrahedral, 2=tetrahedral, 3=trigonal planar
E) 1=trigonal planar, 2=trigonal pyramidal, 3=trigonal pyramidal
20) Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms
in each molecule.
SeO2 SeCl6 SeF2
A) SeCl6 < SeF2 < SeO2
B) SeF2 < SeO2 < SeCl6
C) SeF2 < SeCl6 < SeO2
D) SeO2 < SeF2 < SeCl6
E) SeCl6 < SeO2 < SeF2
21) Place the following in order of increasing F-A-F bond angle, where A represents the central atom in
each molecule.
PF3 OF2 PF4⁺
A) PF3 < OF2 < PF4⁺
B) OF2 < PF3 < PF4⁺
C) OF2 < PF4⁺ < PF3
D) PF4⁺ < OF2 < PF3
E) PF4⁺ < PF3 < OF2
22) Place the following in order of decreasing X-A-X bond angle, where A represents the central atom
and X represents the outer atoms in each molecule.
N2O NCl3 NO2⁻
A) NCl3 > NO2⁻ > N2O
B) NO2⁻ > N2O > NCl3
C) N2O > NO2⁻ > NCl3
D) NCl3 > N2O > NO2⁻
E) N2O > NCl3 > NO2⁻
23) Place the following in order of decreasing X-A-X bond angle, where A represents the central atom
and X represents the outer atoms in each molecule.
CS2 CF4 SCl2
A) CS2 = SCl2 > CF4
B) SCl2 > CF4 > CS2
C) CF4 > CS2 > SCl2
D) CS2 > CF4 > SCl2
E) CF4 > CS2 > SCl2
24) Place the following in order of increasing X-A-X bond angle, where A represents the central atom
and X represents the outer atoms in each molecule.
HCN H2O H3O⁺
A) H2O < H3O⁺ < HCN
B) H3O⁺ < H2O < HCN
C) HCN < H3O⁺ < H2O
D) H2O < HCN < H3O⁺
E) H2O < H3O⁺ < HCN
25) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO3.
A) eg=tetrahedral, mg=trigonal pyramidal, polar
B) eg=tetrahedral, mg=tetrahedral, nonpolar
C) eg=trigonal planar, mg=trigonal planar, nonpolar
D) eg= trigonal bipyramidal, mg=trigonal planar, polar
E) eg=trigonal pyramidal, mg=bent, nonpolar
26) How many of the following molecules are polar?
BrCl3 CS2 SiF4 SO3
A) 1
B) 2
C) 3
D) 4
E) 0
27) How many of the following molecules are polar?
PCl5 COS XeO3 SeBr2
A) 2
B) 0
C) 1
D) 3
E) 4
28) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO2.
A) eg=tetrahedral, mg=bent, polar
B) eg=trigonal planar, mg=bent, polar
C) eg=linear, mg=linear, nonpolar
D) eg=tetrahedral, mg=tetrahedral, nonpolar
E) eg=trigonal pyramidal, mg=trigonal pyramidal, polar
29) Determine the electron geometry (eg), molecular geometry (mg), and polarity of PCl3.
A) eg=tetrahedral, mg=bent, polar
B) eg=trigonal planar, mg=trigonal planar, nonpolar
C) eg=linear, mg=linear, nonpolar
D) eg=tetrahedral, mg=trigonal pyramidal, polar
E) eg=trigonal pyramidal, mg=trigonal pyramidal, polar
30) Determine the electron geometry, molecular geometry and polarity of SF6.
A) eg=trigonal bipyramidal, mg=trigonal bipyramidal, nonpolar
B) eg=tetrahedral, mg=tetrahedral, polar
C) eg=trigonal bipyramidal, mg=see-saw, polar
D) eg=octahedral, mg=trigonal bipyramidal, nonpolar
E) eg=octahedral, mg=octahedral, nonpolar
31) Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3.
A) eg=trigonal planar, mg=trigonal planar, nonpolar
B) eg=tetrahedral, mg=trigonal pyramidal, polar
C) eg=trigonal planar, mg=trigonal pyramidal, polar
D) eg=trigonal bipyramidal, mg=trigonal planar, nonpolar
E) eg=octahedral, mg=tetrahedral, nonpolar
32) Determine the electron geometry, molecular geometry and polarity of HBrO2.
A) eg=trigonal bipyramidal, mg=trigonal planar, nonpolar
B) eg=octahedral, mg=square planar, nonpolar
C) eg=tetrahedral, mg=trigonal pyramidal, polar
D) eg=tetrahedral, mg=linear, nonpolar
E) eg=linear, mg=linear, polar
33) Place the following in order of increasing dipole moment.
I. BCl3 II. BIF2 III. BClF2
A) I < II = III
B) II < III < I
C) I < II < III
D) II < I < III
E) I < III < II
34) Place the following in order of decreasing dipole moment.
I. cis-CHCl=CHCl II. trans-CHCl=CHCI III. cis-CHF=CHF
A) III > I > II
B) II > I > III
C) I > III > II
D) II > III > I
E) I = III > II
35) Identify the number of electron groups around a molecule with sp hybridization.
A) 1
B) 2
C) 3
D) 4
E) 5
36) Identify the number of electron groups around a molecule with sp2 hybridization.
A) 1
B) 2
C) 3
D) 4
E) 5
37) Identify the number of electron groups around a molecule with a tetrahedral shape.
A) 1
B) 2
C) 3
D) 4
E) 5
38) Identify the number of electron groups around a molecule with a trigonal bipyramidal shape.
A) 1
B) 2
C) 3
D) 4
E) 5
39) Identify the number of electron groups around a molecule with an octahedral shape.
A) 6
B) 2
C) 3
D) 4
E) 5
40) Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3.
A) eg=tetrahedral, mg=trigonal planar, sp2
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=tetrahedral, mg=trigonal pyramidal, sp3
D) eg=trigonal pyramidal, mg=tetrahedral, sp3
E) eg=trigonal planar, mg=trigonal planar, sp2
41) Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O.
A) eg=tetrahedral, mg=bent, sp3
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=tetrahedral, mg=trigonal pyramidal, sp3
D) eg=bent, mg=bent, sp2
E) eg=trigonal planar, mg=trigonal planar, sp2
42) Give the electron geometry (eg), molecular geometry (mg), and hybridization for XeF4.
A) eg=tetrahedral, mg=tetrahedral, sp3
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=octahedral, mg=square planar, sp3d2
D) eg=octahedral, mg=octahedral, sp3d2
E) eg=trigonal bipyramidal, mg=seesaw, sp3d
43) Give the hybridization for the O in OF2.
A) sp
B) sp3
C) sp2
D) sp3d
E) sp3d2
44) Give the hybridization for the O in H3O+.
A) sp
B) sp3
C) sp2
D) sp3d
E) sp3d2
45) Give the hybridization for the S in SO3.
A) sp
B) sp3
C) sp2
D) sp3d
E) sp3d2
46) Give the hybridization for the Br in BrO4⁻.
A) sp
B) sp3d2
C) sp3d
D) sp3
E) sp2
47) Give the hybridization for the S in SF6.
A) sp
B) sp2
C) sp3
D) sp3d
E) sp3d2
48) Give the hybridization for the Br in BrF5.
A) sp3d2
B) sp3d
C) sp3
D) sp2
E) sp
49) Give the hybridization for the Br in BrCl3.
A) sp3d2
B) sp3d
C) sp3
D) sp2
E) sp
50) Give the hybridization for the C in HCN.
A) sp3d2
B) sp3d
C) sp3
D) sp2
E) sp
51) Give the hybridization for the C in HCCH.
A) sp3d2
B) sp3d
C) sp3
D) sp2
E) sp
52) How many of the following molecules have sp2 hybridization on the central atom?
HCN SO2 OCl2 XeCl2
A) 4
B) 3
C) 2
D) 1
E) 0
53) Which of the following statements is TRUE?
A) The total number of molecular orbitals formed doesn't always equal the number of atomic orbitals in
the set.
B) A bond order of 0 represents a stable chemical bond.
C) When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will
be lower in energy than the two separate atomic orbitals and one molecular orbital will be higher in
energy than the separate atomic orbitals.
D) Electrons placed in antibonding orbitals stabilize the ion/molecule.
E) All of the above are true.
54) Use the molecular orbital diagram shown to determine which of the following is most stable.
A) F2
B) F22⁺
C) Ne22⁺
D) O22⁺
E) F22⁻
55) Use the molecular orbital diagram shown to determine which of the following are paramagnetic.
A) O22⁻
B) Ne22⁺
C) O22⁺
D) F22⁺
E) None of the above are paramagnetic.
56) Use the molecular orbital diagram shown to determine which of the following is most stable.
A) C22⁺
B) N22⁺
C) B2
D) C22⁻
E) B22⁺
57) Use the molecular orbital diagram shown to determine which of the following are paramagnetic.
A) B22⁺
B) B22⁻
C) N22⁺
D) C22⁻
E) B2
58) Draw the molecular orbital diagram shown to determine which of the following is most stable.
A) F2
B) F22⁺
C) Ne22⁺
D) O22⁺
E) F22⁻
