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Chapter 10 Chemical Bonding II Molecular Geometry and
Hybridization of Atomic Orbitals
Student: ___________________________________________________________________________
2.
The shape of the SF4 molecule is
A.
B.
C.
D.
E.
4.
According to VSEPR theory, the shape of the PH3 molecule is best described as
A.
B.
C.
D.
E.
6.
linear.
trigonal planar.
tetrahedral.
bent.
trigonal pyramidal.
The shape of the ClF3 molecule is best described as
A.
B.
C.
D.
E.
8.
tetrahedral.
trigonal pyramidal.
trigonal planar.
square planar.
distorted tetrahedron (seesaw).
distorted tetrahedron.
trigonal planar.
tetrahedral.
T-shaped.
trigonal pyramidal.
According to the VSEPR theory, the molecular shape of beryllium chloride is
A.
B.
C.
D.
E.
linear.
trigonal planar.
bent.
tetrahedral.
trigonal pyramidal.
10. According to the VSEPR theory, the molecular shape of boron trichloride is
A.
B.
C.
D.
E.
linear.
trigonal planar.
bent.
tetrahedral.
trigonal pyramidal.
12. According to the VSEPR theory, which one of the following species should be linear?
A.
B.
C.
D.
E.
H2S
HCN
BF3
H2CO
SO2
14. According to VSEPR theory, which one of the following molecules should be nonlinear?
A.
B.
C.
D.
E.
CO2
C2H2
SO2
BeCl2
KrF2
16. Which one of the following molecules has tetrahedral geometry?
A.
B.
C.
D.
E.
XeF4
BF3
AsF5
CF4
NH3
18. Predict the geometry around the central atom in PO43-.
A.
B.
C.
D.
E.
trigonal planar
trigonal pyramidal
tetrahedral
trigonal bipyramidal
octahedral
20. Predict the geometry around the central atom in XeO4.
A.
B.
C.
D.
E.
trigonal planar
trigonal pyramidal
tetrahedral
trigonal bipyramidal
octahedral
22. Which of the following substance is/are planar?
(i) SO3
A.
B.
C.
D.
E.
(ii) SO32-
(iii) NO3-
(iv) PF3
(v) BF3
only (i) and (ii)
only (i), (iii), and (v)
only (iv)
all are planar except (iv)
all are planar except (ii)
24. The F-S-F bond angles in SF6 are
A.
B.
C.
D.
E.
90 and 180.
109.5.
120.
180.
90 and 120.
26. According to the VSEPR theory, the actual F-As-F bond angles in the AsF4- ion are predicted to be
A.
B.
C.
D.
E.
109.5.
90 and 120.
180.
< 109.5.
< 90 and < 120.
28. Which one of the following molecules is nonpolar?
A.
B.
C.
D.
E.
NH3
OF2
CH3Cl
H2O
BeCl2
30. Which one of the following molecules has a non-zero dipole moment?
A.
B.
C.
D.
E.
BeCl2
Br2
BF3
IBr
CO2
32. Which one of the following molecules is polar?
A.
B.
C.
D.
E.
PBr5
CCl4
BrF5
XeF2
XeF4
34. Predict the geometry and polarity of the CS2 molecule.
A.
B.
C.
D.
E.
linear, polar
linear, nonpolar
tetrahedral, nonpolar
bent, nonpolar
bent, polar
36. Indicate the type of hybrid orbitals used by the central atom in PCl3.
A.
B.
C.
D.
E.
sp
sp2
sp3
sp3d
sp3d2
38. Indicate the type of hybrid orbitals used by the central atom in SF6.
A.
B.
C.
D.
E.
sp
sp2
sp3
sp3d
sp3d2
40. What is the hybridization on the central atom in NO3- ?
A.
B.
C.
D.
E.
sp
sp2
sp3
sp3d
sp3d2
42. What is the hybridization of As in the AsF4- ion?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
44. The hybridization of the central nitrogen atom in the molecule N2O is
A.
B.
C.
D.
E.
sp.
sp2.
sp3.
sp3d.
sp3d2.
46. In which of these molecules do the two nitrogen atoms have different hybridizations?
A.
B.
C.
D.
E.
NH4NO3
N2H4
N2O4
N2O5
none of these
48. Which of the following molecules have the same geometries?
A.
B.
C.
D.
SF4 and CH4
CO2 and H2O
CO2 and BeH2
N2O and NO2
50. The number of pi bonds in the molecule below is
A.
B.
C.
D.
E.
2.
4.
6.
10.
15.
52. Consider the species Cl2+, Cl2, and Cl2-. Which of these species will be paramagnetic?
A.
B.
C.
D.
E.
Only Cl2
Cl2+ and Cl2
Cl2 and Cl2Cl2+ and Cl2All three are paramagnetic.
54. In which of the following would the bonding be strengthened with the addition of an electron to form the
negative molecular ion?
A.
B.
C.
D.
E.
N2
O2
F2
all of these
none of these
56. In which of the following would the bonding be weakened with the addition of an electron to form the
negative molecular ion?
A.
B.
C.
D.
E.
B2
C2
N2
all of these
none of these
58. Which of the following is not true of molecular orbitals?
A.
B.
C.
D.
E.
The number of molecular orbitals formed is always equal to the number of atomic orbitals combined.
A molecular orbital can accommodate up to two electrons.
When electrons are added to orbitals of the same energy, the most stable arrangement is predicted by
Hund's rule.
Low-energy molecular orbitals fill before high-energy molecular orbitals fill.
For any substance, the number of electrons in molecular orbitals is equal to the sum of all the valence
electrons on the bonding atoms.
60. Which of the following correctly lists species in order of increasing bond length?
A.
B.
C.
D.
E.
O2 < O2+ < O2O2- < O2 < O2+
O2+ < O2 < O2O2- < O2+ < O2
O2+ < O2- < O2
62. Which of the following correctly lists species in order of increasing bond order?
A.
B.
C.
D.
E.
C2 < Li2 < Be2 < N2
Be2 < Li2 < C2 < N2
N2 < Be2 < Li2 < C2
N2 < C2 < Li2 < Be2
Be2 < C2 < N2 < Li2
Chapter 10 Chemical Bonding II Molecular Geometry and
Hybridization of Atomic Orbitals Key
2.E
4.E
6.D
8.A
10.B
12.B
14.C
16.D
18.C
20.C
22.B
24.A
26.E
28.E
30.D
32.C
34.B
36.C
38.E
40.B
42.D
44.A
46.A
48.C
50.B
52.D
54.E
56.C
58.E
60.C
62.B