Question

hybridisation of cl in clo2-

Answer 1

clo2- here cl is the central atom bonded to 2 oxygen atom and after bonding it has 2 lone pair of electron including negative one.according to formula AB2L2 then 2+2=4=sp3

Answer 2

Answer : The hybridization of Cl in $ClO_2^-$ is $sp^3$

Explanation :

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 $ClO_2^-$ molecules.

$\text{Number of electrons}=\frac{1}{2}\times [7+1]=4$

Bond pair electrons = 2

Lone pair electrons = 4 - 2 = 2

The number of electrons are 4 that means the hybridization will be $sp^3$ and the electronic geometry of the molecule will be tetrahedral.

But as there are two atoms around the central chlorine atom, the third and fourth 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 bent.