Why does elemental silicon not form a graphite-like structure, whereas carbon does?

Explanation

In graphite carbon is `sp^2` hybridese and each carbon forms convalent bonds with three carbon atoms and forms extende hexaogonal rign -Like structure in the layer . Each carbon is now left with one unpaird electron in unhyridsed `2p` orbital which undrgoes sidways ovelap to form `p pi- p pi` double bonds . Thus , graphite has a two-dimensional sheet-like (alyered) stuture .
On the other hand Si is not capable of forming structure like fraphite. Due to its bigger size. exteny of overlap , which cannot form `Si = Si`. Rather. Si prefes to undrgo `sp^3` hdycridisation and hence silicon has a diamond-like three-dimensional netword structure
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