Carbon and silicon belong to group IV. The ma | vedclass

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(C) Carbon $(C)$ has the electronic configuration $2s^2 2p^2$ and lacks $d$-orbitals in its valence shell,limiting its covalency to $4$.Silicon $(Si)$

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Availability of low lying $d$-orbitals in silicon

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(C) Carbon $(C)$ has the electronic configuration $2s^2 2p^2$ and lacks $d$-orbitals in its valence shell,limiting its covalency to $4$.Silicon $(Si)$ has the electronic configuration $3s^2 3p^2$ and possesses vacant $3d$-orbitals.Due to the availability of these low-lying vacant $d$-orbitals,silicon can expand its octet and accommodate more ligands,allowing it to exhibit a coordination number of $6$ (e.g.,in $[SiF_6]^{2-}$).

Carbon and silicon belong to group $IV$. The maximum coordination number of carbon in commonly occurring compounds is $4$,whereas that of silicon is $6$. This is due to

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