Chapter 14: Q14.20E (page 599)
Give the expected hybridization of the central atom for the molecules in Exercises 99 and 100 from Chapter 13.
The expected hybridization of the central atom for the molecules are given below.
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Arrange the following from lowest to highest ionization energy: . Explain your answer.
Question: In terms of the molecule orbital model which species in each of the following two pairs will most likely be the one to gain an electron? Explain. CN or NO or or
Describe the bonding in the first excited state of N2 (the one closest in energy to the ground state) using the MO model. What differences do you expect in the properties of the molecule in the ground state and in the first excited state? (An excited state of a molecule corresponds to an electron arrangement other than that giving the lowest possible energy.)
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- .
In exercise 71 in chapter 13 the lewis structure for benzene was drawn. Using one of the lewis structures estimate for . Using bond energies and given standard enthalpies of formation of C(g) is 717kJ/mol. The experimental for is 83 kJ/mol. Explain the discrepancy between the experimental value and the calculated value of .
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