Chemistry - CHEMICAL BONDING Question with Solution | TestHub

The central atom in ${\text{ClF}}_3$ is Chlorine (Cl).

Number of valence electrons of Cl = $7$.

Number of monovalent atoms (F) attached = $3$.

Steric number = $\frac{1}{2}(7+3)=5$.

The hybridization of the central atom is $s{p}^{3}d$.

Number of bond pairs = $3$.

Number of lone pairs = $5-3=2$.

The electron geometry is trigonal bipyramidal. According to VSEPR theory, to minimize repulsion, the two lone pairs occupy the equatorial positions.

This results in a T-shaped molecular geometry.

Therefore, ${\text{ClF}}_3$ has a T-shaped geometry with two lone pairs on the Cl atom.

Answer: It has T-shaped geometry with two lone pairs on Cl atom.