C - C bond length in graphite is shorter than C - C bond length in diamond - Explain.

Explanation

In graphite each carbon is in `sp^2` hybridisation and makes three sigma bonds with three neighbouring carbon atoms. Fourth electron forms a `pi` Bond. The electron is delocalised over the whole sheet. Due to this C - C bond length is shorter in graphite. In diamond each carbon is in `sp^3` hybridisation. So every carbon forms four `C - C ` single bonds. `sp^2-sp^2` bond is stronger than `sp^3 -sp^3` bond. Hence C - C bond length in diamond is longer than in graphite.