Choose the polar molecule from the following:

Question

Canvas Classes · Accepted Answer

A polar molecule has a net dipole moment (asymmetric charge distribution).

Step 1 — Analyse each molecule:

- : Tetrahedral, all C–Cl bonds cancel → zero dipole moment (non-polar) ✗
- : Linear, two C=O bonds cancel → zero dipole moment (non-polar) ✗
-  (ethene): Symmetric planar structure → zero dipole moment (non-polar) ✗
-  (chloroform): Tetrahedral but asymmetric — 3 Cl and 1 H → bond dipoles do NOT cancel → net dipole moment (polar) ✓

Answer: Option (4) —

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