Concept:The carbonyl group (\( >C=O \)) is highly polar due to the electronegativity difference between carbon and oxygen.
Solution:- Oxygen is significantly more electronegative than carbon.
- While both the \( \sigma \) and \( \pi \) bonds are polarized, the electrons in the \( \pi \) bond are held more loosely (side-to-side overlap) compared to the tightly held \( \sigma \) bond electrons (head-to-head overlap).
- Therefore, the electron cloud of the \( \pi \) bond is strongly distorted (pulled) towards the highly electronegative oxygen atom, creating a permanent dipole.
Why other options are incorrect:The \( \sigma \) bond is more rigid and less polarizable. \( C-H \) and \( C-C \) bonds are virtually non-polar compared to the \( C=O \) bond.
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