No form fo elecmental silicon is comparabnle to graphite Give reason .

Explanation

In graphite, carbon is `sp^(2)`-hybridized and each carbon is liked to three other carbon atoms by forming hexagonal rings. Each carbon is now left with on unhybridized p-orbital which undergoes sideways overlap to form three `ppi-ppi` double bonds. Thus, graphite has two dimensional sheet like (layered) structure consisting of a number of benzene rings fused together . Silicon on the other hand, does not forman anlogue of carbon because of the following reason :
Due to bigger size kand smaller electronegativity of Si than C, it does not undergo `sp^(2)`-hybridization and hence it does not form `ppi-ppi` double bonds needed for graphite like structure . Instead , it prefers to undergo only `sp^(3)`-hybridization and hence silicon has diamond like three-dimensional network structure.