Among SO2, NF3, NH3, XeF2, ClF3 and SF4, the hybridization of the molecule with non-zero dipole moment and highest…

🧠 Find the species with non-zero dipole moment and the highest number of lone pairs on the central atom, then give its hybridization.

🗺️ Step 1 — Lone pairs and dipole moments:

| Molecule | Shape | LP on central atom | Dipole moment | |----------|-------|-------------------|--------------| | $\ce{SO2}$ | Bent | 1 | ≠ 0 ✓ | | $\ce{NF3}$ | Pyramidal | 1 | ≠ 0 ✓ | | $\ce{NH3}$ | Pyramidal | 1 | ≠ 0 ✓ | | $\ce{XeF2}$ | Linear | 3 | = 0 ✗ | | $\ce{ClF3}$ | T-shaped | 2 | ≠ 0 ✓ | | $\ce{SF4}$ | See-saw | 1 | ≠ 0 ✓ |

Step 2 — Among polar molecules, highest LP on central:

$\ce{ClF3}$: 2 lone pairs on Cl → highest LP among polar molecules ✓

Step 3 — Hybridization of $\ce{ClF3}$:

Cl: 3 bonds + 2 LP = 5 electron pairs → $sp^3d$ hybridization

$\boxed{\text{Answer: } sp^3d}$