If lone pairs of electrons occupy axial posit | vedclass

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(C) The central atom $Cl$ in $ClF_3$ has $7$ valence electrons. It forms $3$ $Cl-F$ bonds and has $2$ lone pairs,resulting in $sp^3d$ hybridization.Ac

Vedclass · Accepted Answer

All bond lengths are equal

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(C) The central atom $Cl$ in $ClF_3$ has $7$ valence electrons. It forms $3$ $Cl-F$ bonds and has $2$ lone pairs,resulting in $sp^3d$ hybridization.According to $VSEPR$ theory,lone pairs occupy equatorial positions to minimize $lp-lp$ and $lp-bp$ repulsions.If the lone pairs were to occupy axial positions,the $lp-lp$ repulsion would be higher,and the molecule would not be stable in that configuration.In the actual $T$-shaped structure,the two axial $Cl-F$ bonds are longer than the equatorial $Cl-F$ bond due to the repulsion from the lone pairs.Therefore,the statement that 'All bond lengths are equal' is incorrect.

If lone pairs of electrons occupy axial positions,then which of the following statements about $ClF_3$ is incorrect?

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