JEE Main · 2025 · 02 Apr 2025 · Shift 1 · Chemical Bonding and Molecular Structure

Each species is weighed for a non-zero dipole and for lone pairs on the central atom: $\mathrm{SO}{}_2$ is bent ($s{p}^2$, one lone pair, polar); $\mathrm{NF}{}_3$ and $\mathrm{NH}{}_3$ are pyramidal ($s{p}^3$, one lone pair, polar); $\mathrm{XeF}{}_2$ is linear ($s{p}^{3}d$, three lone pairs, but non-polar); $\mathrm{ClF}{}_3$ is T-shaped ($s{p}^{3}d$, two lone pairs, polar); $\mathrm{SF}{}_4$ is see-saw ($s{p}^{3}d$, one lone pair, polar). Among the polar molecules the largest number of lone pairs, two, sits on the chlorine of $\mathrm{ClF}{}_3$, whose central atom is $s{p}^{3}d$ hybridised.