The hybrid orbitals used by central atoms in | vedclass

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(B) To determine the hybridisation,we calculate the number of electron pairs around the central atom using the formula: $	ext{Number of hybrid orbita

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$sp$,$sp^2$ and $sp^3$

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(B) To determine the hybridisation,we calculate the number of electron pairs around the central atom using the formula: $	ext{Number of hybrid orbitals} = 	ext{Number of sigma bonds} + 	ext{Number of lone pairs}$.In $BeCl_2$,$Be$ has $2$ sigma bonds and $0$ lone pairs,so it is $sp$ hybridised.In $BCl_3$,$B$ has $3$ sigma bonds and $0$ lone pairs,so it is $sp^2$ hybridised.In $CCl_4$,$C$ has $4$ sigma bonds and $0$ lone pairs,so it is $sp^3$ hybridised.Therefore,the hybrid orbitals are $sp$,$sp^2$ and $sp^3$ respectively.

The hybrid orbitals used by central atoms in $BeCl_2$,$BCl_3$ and $CCl_4$ molecules are respectively

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