1. In ozone, O3, the two oxygen atoms on the ends of the molecule are equivalent to one another.
(a)What is the best choice of hybridization scheme for the atoms of ozone?
(b) For one of the resonance forms of ozone, which of the orbitals are used to make bonds and which are used to hold nonbonding pairs of electrons?
(c) Which of the orbitals can be used to delocalize the π electrons?
(d) How many electrons are delocalized in the π system of ozone?
2. Butadiene, C4H6, is a planar molecule that has the following carbon-carbon bond lengths:
(a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) Compare the bond lengths to the average bond lengths listed in Table 8.5. Can you explain any differences?
Table: Average Bond Lengths for Some Single, Double, and Triple Bonds
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Bond
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Bond Length (A)
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Bond
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Bond Length (A)
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C-C
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1.54
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N-N
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1.47
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C=C
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1.34
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N=N
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1.24
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C=C
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1.20
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N=N
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1.10
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C-N
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1.43
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N-0
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1.36
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C=N
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1.38
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N=0
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1.22
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C=N
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1.16
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0-0
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1.48
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C-0
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1.43
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0=0
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1.21
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C=0
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1.23
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C=0
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1.13
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