Carbons in graphite and benzene both exhibit sp2 hybridization with one leftover 2p electron. What is the difference in the function of the 2p electron in graphite versus the 2p electron in benzene? a. There is no difference. The 2p electrons form and break double covalent bonds with other carbons in the compound.
b. The 2p electrons in benzene are delocalized to form the resonance structure, but the 2p electrons in graphite are not delocalized, and they form single sigma bonds with other carbons.
c. The delocalized 2p electrons in graphite help the graphite layers stick together electrostatically while in benzene the 2p electrons form resonant double bonds.
d. The 2p electron in graphite jumps to a higher energy level to form carbon bonds characteristic of a diamond, while the 2p electron in benzene forms a strong single bond with a neighboring carbon.