A central atom in a molecule has two lone pai | vedclass

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(C) The total number of electron pairs around the central atom is the sum of the number of bond pairs and lone pairs.Total electron pairs = $3$ (bond

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$T$-shaped

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(C) The total number of electron pairs around the central atom is the sum of the number of bond pairs and lone pairs.Total electron pairs = $3$ (bond pairs) + $2$ (lone pairs) = $5$.According to $VSEPR$ theory,a total of $5$ electron pairs corresponds to $sp^3d$ hybridization with a trigonal bipyramidal electron geometry.When there are $3$ bond pairs and $2$ lone pairs,the lone pairs occupy the equatorial positions to minimize repulsion.This results in a $T$-shaped molecular geometry.

$A$ central atom in a molecule has two lone pairs of electrons and forms three single bonds. The shape of this molecule is

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