See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Resonance Energy Comparison **Resonance energy** is the stabilization gained from delocalization of π electrons. It increases with: - More effective orbital overlap - Better stabilization of negative charge on electronegative atoms - Stronger conjugation ## Analysis of Each Molecule: **I. $CH_2 = CH - F$** - Fluorine is highly electronegative but has poor orbital overlap with the adjacent C=C π system (small p-orbital, high electronegativity mismatch) - Minimal resonance contribution - **Lowest resonance energy** **II. $CH_2 = CH - OH$** - Oxygen is electronegative with suitable orbital size for overlap - Lone pairs on O can delocalize effectively into the π system - Forms resonant structures with negative charge well-stabilized on oxygen - **High resonance energy** **III. $CH_2 = CH - NH_2$** - Nitrogen has lone pairs available for delocalization - More effective π-donor than oxygen (less electronegative, better orbital matching) - Nitrogen lone pairs delocalize strongly into conjugated system - Forms more stable resonant structures - **Highest resonance energy** ## Order: $$\text{III} > \text{II} > \text{I}$$ **The answer is (B):** Nitrogen's superior donor ability and orbital characteristics make it the strongest resonance stabilizer, followed by oxygen, then fluorine's poor overlap contribution.