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InterviewSolution
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Why does not silicon form an analogue of graphite ? |
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Answer» 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. |
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