Like cyclohexane (Problem 8.54), benzene also contains a sixmembered ring of carbon atoms, but it is flat rather than puckered. Explain, and predict the values of the C¬C¬C bond angles.

Hybridization is the concept that describes the mixing of atomic orbitals to form new hybrid orbitals, which can explain the geometry of molecular structures. In benzene, each carbon atom undergoes sp² hybridization, resulting in three sp² hybrid orbitals that form sigma bonds with adjacent carbon atoms and hydrogen atoms, while the remaining unhybridized p orbital contributes to the delocalized pi bonding system.

Benzene is a planar molecule due to the sp² hybridization of its carbon atoms, which allows for the formation of a flat, cyclic structure. The arrangement minimizes steric strain and maximizes overlap of p orbitals, leading to resonance stabilization. This planarity is crucial for the delocalization of electrons, which contributes to benzene's unique stability and reactivity.

In benzene, the C-C-C bond angles are predicted to be approximately 120 degrees due to the trigonal planar arrangement of the sp² hybridized carbon atoms. This angle is characteristic of sp² hybridization, where the orbitals are arranged to minimize electron pair repulsion, resulting in a flat structure that supports the delocalization of pi electrons across the ring.