Carbonyl compounds have a planar structure with a π-bond, leading to substantial dipole moments. The high polarity is explained by resonance, involving neutral (A) and dipolar (B) structures, contributing to the overall dipole moment of carbonyl compounds.
What structural characteristics contribute to the high polarity of carbonyl compounds compared to ethers, and how is this polarity explained through resonance?
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The high polarity of carbonyl compounds compared to ethers is attributed to the presence of a carbon-oxygen double bond in the carbonyl group. In carbonyl compounds, the oxygen is more electronegative, resulting in a significant dipole moment. This polarity is explained through resonance, where the π electrons can delocalize between the carbon and oxygen atoms, creating a resonance hybrid. The resonance forms depict partial double-bond character on oxygen, increasing its electron density. This resonance stabilization reinforces the polarity, making carbonyl compounds more polar than ethers, where the oxygen is involved in a single bond and lacks resonance stabilization.