In ClF_3 molecule,if the lone pair of the cen | vedclass

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(D) The $ClF_3$ molecule has $sp^3d$ hybridization with $2$ lone pairs and $3$ bond pairs. According to $VSEPR$ theory,lone pairs occupy equatorial po

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(D) The $ClF_3$ molecule has $sp^3d$ hybridization with $2$ lone pairs and $3$ bond pairs. According to $VSEPR$ theory,lone pairs occupy equatorial positions to minimize repulsion. If the lone pairs were to occupy axial positions,the molecule would adopt a $T$-shaped geometry with a $120^o$ bond angle between the equatorial fluorine atoms. In this hypothetical configuration,the molecule would be non-polar due to the symmetric arrangement of the polar $Cl-F$ bonds,and the shape would be trigonal planar. Since all these statements describe the consequences of the lone pairs occupying axial positions,the correct option is $D$.

Molecule	Geometry
$(a) SnCl_2$	$(i)$ Angular (or) Bent
$(b) XeF_4$	$(ii)$ See-saw
$(c) ClF_3$	$(iii)$ Square pyramidal
$(d) IF_5$	$(iv)$ $T$-shape
-	$(v)$ Square planar

In $ClF_3$ molecule,if the lone pair of the central atom occupied the axial position,then which of the following statements is correct?

Similar Questions

Match the following?
Molecule Geometry
$(a) SnCl_2$ $(i)$ Angular (or) Bent
$(b) XeF_4$ $(ii)$ See-saw
$(c) ClF_3$ $(iii)$ Square pyramidal
$(d) IF_5$ $(iv)$ $T$-shape
- $(v)$ Square planar

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