Why does not sillicon form an analogue of graphite?

Answer

In graphite, carbon is `sp^(2)`-hybridized and each carbon is linked to three other carbon atoms by forming hexagonal rings.Each carbon is now left with one 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 form an analogue of carbon because of the following reason:
Due to bigger size and 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 perfers to undergo only `sp^(3)`-hybridization and hence silicon has diamond like three-dimensional network structure.