Explain the molecular orbital structure of benzene .

Explanation

The structure of benzene is best described in terms of the molecular orbital theory. All the six carbon atoms of benzene are `sp^(2)` hybridized. Six `sp^(2)` hybrid orbitals of carbon linearly overlap with six one is orbitals of hydrogen atoms to form six `C-H` sigma bonds. Overlap between the remaining `sp^(2)` hybrid orbitals of carbond forms six `C-C` sigma bonds.
All the bonds in benzene lie in one plane with bond angle `120^(@)`. Each carbon atom in benzene possess an un hybridized `p`-orbital containing one electron. The lateral overlap of their `p`-orbital produces `3pi` bond The six electrons of the `p`-orbitals cover all the six carbon atoms and are said to be delocalised.
Due to delocalization, strong -bond is formed which makes the molecule stable. Hence unlike alkenes and alkynes benzene undergoes substitution reactions rather addition reactions under normal conditions.