Question

Match the molecules/ions (in Column-I) with their shapes (in Column-II).

Answer 1

(A) $Cl{F}_3$ is $s{p}^{3}d$ hybridized with two lone pair of electrons. Thus, geometry is T-shaped structure with two axial and one equatorial bonds.

(B). ${\left[P{Cl}_4\right]}^{+}$ is $s{p}^3$ hybridized with tetrahedral geometry.

(C) $Xe{F}_4$ is $s{p}^3{d}^2$ hybridized with expected geometry octahedral but due to presence of 2 lone pairs, the geometry is square planar.

(D) $Xe{O}_3$ is $s{p}^3$ hybridized with expected geometry is pyramidal.