What is the shape of the ClF_3 molecule? | vedclass

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(C) To determine the shape of the $ClF_3$ molecule,we calculate the number of electron pairs around the central atom $Cl$ using the formula: $X = \fra

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$T$-shaped

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(C) To determine the shape of the $ClF_3$ molecule,we calculate the number of electron pairs around the central atom $Cl$ using the formula: $X = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electrons of the central atom $(Cl = 7)$,$M$ is the number of monovalent atoms $(F = 3)$,$C$ is the cationic charge $(0)$,and $A$ is the anionic charge $(0)$.$X = \frac{1}{2} [7 + 3] = 5$.This indicates $sp^3d$ hybridization.Out of $5$ electron pairs,$3$ are bond pairs (forming $3$ $\sigma$-bonds with $F$ atoms) and $2$ are lone pairs.According to $VSEPR$ theory,the $2$ lone pairs occupy the equatorial positions to minimize repulsion,resulting in a $T$-shaped molecular geometry.

What is the shape of the $ClF_3$ molecule?

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