What is the hybridisation of each carbon atom in benzene?

Each carbon atom in benzene is sp² hybridised. Benzene has the molecular formula C₆H₆ and forms a planar hexagonal ring. Every carbon uses three sp² hybrid orbitals to make three sigma bonds: two with neighbouring carbon atoms and one with hydrogen. One unhybridised p orbital remains on each carbon. This delocalisation explains why all carbon–carbon bonds in benzene have the same intermediate length. An sp² carbon has trigonal planar geometry with bond angles close to 120°. Concept depth: In benzene, every carbon is bonded to two neighbouring carbon atoms and one hydrogen atom through three sigma bonds. One unhybridised p orbital remains perpendicular to the ring on each carbon.