Which one of the following molecules has maximum dipole moment?

Question

Canvas Classes · Accepted Answer

Dipole moment depends on bond polarity and molecular geometry.

Step 1 — Analyse each molecule:

- : Tetrahedral, symmetric → zero dipole moment ✗
- : Trigonal bipyramidal, symmetric → zero dipole moment ✗
- : Pyramidal; N–F bonds point away from lone pair; bond dipoles partially cancel lone pair dipole → small dipole moment (~0.24 D)
- : Pyramidal; N–H bonds point toward lone pair; bond dipoles ADD to lone pair dipole → large dipole moment (~1.47 D)

Step 2: In , the lone pair and bond dipoles

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