Final answer:
The bonding in a benzene ring is characterized by sp² hybridized carbon atoms with a delocalized system of pi electrons, resulting in a bond character that is a hybrid between a single and a double bond.
Step-by-step explanation:
The most accurate description of the bonding in a benzene ring involves delocalized electrons and the resonance between two structures. Benzene is characterized by a hexagonal arrangement of carbon atoms, with each carbon atom being sp² hybridized. This arrangement allows for the p orbitals of the carbon atoms to overlap, resulting in a system of delocalized π (pi) electrons shared across all six carbon atoms. The actual bond character is intermediate between that of a C-C single bond and a C=C double bond, which is why representations of benzene often include a circle within the hexagonal structure to indicate the delocalization of pi electrons.
Valence bond theory helps explain the structure by suggesting that each carbon atom has three sp² hybrid orbitals that form sigma bonds, with the remaining p orbital forming the part of the delocalized pi bond system. This theory is substantiated by the fact that all C-C bonds in benzene have a bond length (139.9 pm) that is between that of a single bond (154 pm) and a double bond (134 pm), evidencing their unique hybrid character. The overall structure of benzene is often depicted with single bonds around a hexagon and a circle in the center, highlighting the electron delocalization.