Match List I with List II List I List II A. XeF _ 4 I.See-saw B. SF...

(A) ${XeF}_{4}$:

$Xe$ has 4 bond pairs along with 2 lone pairs in the ${XeF}_{4}$. Thus, the hybridisation of $Xe$ is ${sp}^{3}{d}^{2}$. Now since it contains two lone pairs it will show square planar geometry.

(B) ${SF}_{4}$:

The lone pair is an equatorial position, and there are two lone-pair—bond pair repulsions. Hence, it is more stable. So, the shape is described as a distorted tetrahedron, a folded square or a see-saw.

(C) ${NH}_{4}^{+}$:

In this case steric number = lone pair + sigma bond = 0 + 4 = 4.

So, it is sp³ hybridisation. There is no lone pair present. Thus, the shape of this ion is tetrahedral.

(D) ${BrF}_{3}$:

To decrease repulsion between the lone pairs, the molecule's structure is bent, making it T-shaped.