Question

What is the hybridisation of " XeOF4 "

Answer 1

Explanation:

it's hybridisation is sp³d². It's a bit complex

Answer 2

Answer: The number of electrons are 6 that means the hybridization will be $sp^3d^2$

Explanation:

The example of a square planar molecule is, xenon oxytetrafluoride $(XeOF_4)$.  

Formula used  :

$\text{Number of electrons}=\frac{1}{2}[V+N-C+A]$

where,

V = number of valence electrons present in central atom

N = number of monovalent atoms bonded to central atom

C = charge of cation

A = charge of anion

Now we have to determine the hybridization of the $XeOF_4$ molecule.

$\text{Number of electrons}=\frac{1}{2}\times [8+4]=6$

Bond pair electrons = 4

Lone pair electrons = 5 - 4 = 1

The number of electrons are 6 that means the hybridization will be $sp^3d^2$ and the electronic geometry of the molecule will be octahedral.

But as there are five atoms around the central xenon atom, the sixth position will be occupied by lone pair of electrons. The repulsion between lone and bond pair of electrons is more and hence the molecular geometry will be square pyramidal.