The overlapping of orbitals in benzene is of the type

Options

A. `sp^(2) - sp^(2)`
B. `sp^(3)-sp^(3)`
C. `sp-sp`
D. `p-p`

Answer

D

Explanation

According to molecular orbital theory of benzene, each carbon atom is `sp^2` hybridized with a bond angle of 120º. There are six `2p_3` atomic orbitals (one on each carbon atom) which are parallel to each other but are perpendicular to the plane of the ring and project above and below the plane.
Each `P_x` orbital interacts equally with its two neighbours producing a circular double–doughnut shaped molecular orbital embracing all six carbon atoms and thus six `pi`- electrons are delocalized.