The hybridizations of carbon in graphite, diamond and C 60 are respectively

Step-by-step solution

Diamond, graphite and C 60 are known as allotropes of carbon. In diamond, each carbon atom is tetrahedrally bonded to four carbon atoms, forming a 3 - D network of strong, covalently bonded carbon atoms. All carbon atoms are sp 3 hybridized. While in graphite and C 60 , each carbon is bonded to three carbon atoms, forming a network of hexagonal rings arranged in a plane in graphite and as sphere in C 60 . All carbon atoms are sp 2 hybridized and have one free electron. Numerous such layers are bonded to each other