Chapter 14: Q14.8DQ (page 599)
What are the relationship among bond order, bond energy and bond length? Which of these quantities can be measured?
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The molecule is linear and polar.
a. On the basis of this experimental evidence, which arrangement is correct, NNO or NON? Explain your answer.
b. On the basis of your answer in part a, write the Lewis structure of (including resonance forms). Give the formal charge on each atom and the hybridization of the central atom.
c. How would the multiple bonding in
be described in terms of orbitals?
Question: How does molecular orbital theory explain the following observations?
a. H2 is stable, whereas He2 is unstable.
b. B2 and O2 are paramagnetic, whereas C2 , N2and F2 are diamagnetic.
c. N2 has a very large bond energy associated with it.
d. NO+ is more stable than NO- .
The NMR spectra on the right are for the organic compounds C6H12 and C4H10O. Deduce the structures for these compounds. See Exercise 74 for a discussion of the bonding in organic compounds. The structure of C6H12 has one double bond, with the rest being single bonds, and the structure of C4H10O has only single bonds. Note that the TMS reference has been omitted in each spectrum.
In which of the following diatomic molecules would the bond strength be expected to be weaken as an electron is removed?
a.
b.
c.
d. OF
Values of measured bond energies may vary greatly depending on the molecule studied. Consider the following reactions:
Rationalize the difference in the values offor these reactions, even though each reaction appears to involve the breaking of only one N-Cl bond. (Hint: Consider the bond order of the NO bond in ONCl and in NO.)
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