Question

6. In the Lewis structure of XeF2, how many lone pairs are around the central atom? a. 3 b.4 c. 5 d. 6 e. 2

Answer 1

Answer: The correct answer is Option a.

Explanation:

To calculate the hybridization of central metal atom, we use the equation:

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

where,

V = number of valence electrons present in central atom  which is xenon = 8

N = number of monovalent atoms bonded to central atom  = 2

C = charge of cation  = 0

A = charge of anion  = 0

Putting values in above equation, we get:

$\text{Number of electron pair}=\frac{1}{2}\times [8+2]=5$

The number of electron pair are 5 that means the hybridization will be $sp^3d$ and the electronic geometry of the molecule will be

But as there are 2 atoms around the central xenon atom, rest three positions 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 bent or linear.

Hence, the correct answer is Option a.