Explain the following giving an appropriate reason in each case.
Structures of Xenon fluorides cannot be explained by Valence Bond approach.

According to the valence bond approach, covalent bonds are formed by the overlapping of the half-filled atomic orbital. But xenon has a fully filled electronic configuration. Hence the structure of xenon fluorides cannot be explained by VBT.

For example: In case of XeF₂

Hybridization is:
Total, valence electron =8 for Xe

Monovalent atom F=2

So, total hybrid orbitals =1/2 [valence electron + monovalent atom + cation + anion] as no cation and anion so term is zero

 So hybrid orbital are ½[8+2+0+0] = 5
So hybridization = sp³d

According to sp³d hybridization, the structure should be Trigonal bipyramidal, but the actual structure is linear. So, VBT fails to answer this however VSPER theory explains the liner shape.