For benzene, the total π-electron energy is Eπ = 6α +
8β and for 1,3,5-hexatriene it is Eπ = 6α + 6.99β.
(a) Using Huckel molecular orbital theory, compare the total
π-electron energy of 1,3,5-hexatriene to the energy of a molecule
with 3 localized π-bonds (i.e. 3 ethene molecules). What factor
leads to the lower energy of 1,3,5-hexatriene as compared to the
molecule with 3 localized π-bonds? Explain.
(b) Explain why the total π-electron energies of benzene and
1,3,5-hexatriene are...