Ch05 Molecular Structure and Orbitals.pdf - finedrafts

V
V
V
V
33. Consider the following Lewis structure where E is an unknown
element:
OOEOO A
O
What are some possible identities for element E? Predict the
molecular structure (including bond angles) for this ion.
34. Consider the following Lewis structure where E is an unknown
element:
−
O 2–
D
SOFOO Q QE
G
O
QF
S
What are some possible identities for element E? Predict the
molecular structure (including bond angles) for this ion. (See
Exercises 25 and 26.)
35. The molecules BF 3, CF 4, CO 2, PF 5, and SF 6 are all nonpolar,
even though they all contain polar bonds. Why?
36. Two different compounds have the formula XeF 2Cl 2. Write
Lewis structures for these two compounds, and describe how
measurement of dipole moments might be used to distinguish
between them.
The Localized Electron Model and Hybrid Orbitals
37. Use the localized electron model to describe the bonding in H 2O.
38. Use the localized electron model to describe the bonding in CCl 4.
39. Use the localized electron model to describe the bonding in
H 2CO (carbon is the central atom).
40. Use the localized electron model to describe the bonding in
C 2H 2 (exists as HCCH).
41. The space- lling models of ethane and ethanol are shown below.
Ethane
(C 2H 6)
Ethanol
(C 2H 5OH)
Use the localized electron model to describe the bonding in
ethane and ethanol.
42. The space- lling models of hydrogen cyanide and phosgene
are shown below.
Hydrogen cyanide
(HCN)
Phosgene
(COCl 2)
Use the localized electron model to describe the bonding in
hydrogen cyanide and phosgene.
43. Give the expected hybridization of the central atom for the
molecules or ions in Exercises 75 and 81 from Chapter 4.
44. Give the expected hybridization of the central atom for the
molecules or ions in Exercises 76 and 82 from Chapter 4.
Q
Q
Q
C
H
O
C
H
O
N
Cl
Exercises 235
45. Give the expected hybridization of the central atom for the
molecules in Exercises 21 and 22.
46. Give the expected hybridization of the central atom for the
molecules in Exercises 27 and 28.
47. For each of the following molecules, write the Lewis
structure(s), predict the molecular structure (including bond
angles), give the expected hybrid orbitals of the central atom,
and predict the overall polarity.
a. CF 4 e. BeH 2 i. KrF 4
b. NF 3 f. TeF 4 j. SeF 6
c. OF 2 g. AsF 5 k. IF 5
d. BF 3 h. KrF 2 l. IF 3
48. For each of the following molecules or ions that contain sulfur,
write the Lewis structure(s), predict the molecular structure
(including bond angles), and give the expected hybrid orbitals
for sulfur.
a. SO 2
b. SO 3
c.
d.
O
S 2O 3 2− S S
O
O
O
2−
2− S2O8 O S O O S
O
e. SO 3 2
f. SO 4 2
g. SF 2
h. SF 4
i. SF 6
j. F 3SOSF
k. SF 5
O
49. Why must all six atoms in C 2H 4 lie in the same plane?
50. The allene molecule has the following Lewis structure:
O
O
2−
H
H
G
CPCPC
D
H
H
Must all hydrogen atoms lie the same plane? If not, what is
their spatial relationship? Explain.
51. Indigo is the dye used in coloring blue jeans. The term navy
blue is derived from the use of indigo to dye British naval
uniforms in the eighteenth century. The structure of the indigo
molecule is
H
O
H C C N C H
C C
C C
C C
C C
C C
H C N C C H
H
H
a. How many bonds and bonds exist in the molecule?
b. What hybrid orbitals are used by the carbon atoms in the
indigo molecule?
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D
G
H
O
H
H