Choose the compound which has a maximum bond angle at nitrogen among the following:

Question

Accepted Answer

1. **Analyze NO₂⁺ (Nitronium Ion):**
   - Hybridization: $H = \frac{1}{2}(V + M - C + A) = \frac{1}{2}(5 + 0 - 1 + 0) = 2$ (sp hybridization).
   - Structure: Linear.
   - Bond Angle: **180°**.
2. **Analyze NO₃⁻ (Nitrate Ion):**
   - Hybridization: $H = \frac{1}{2}(5 + 0 - 0 + 1) = 3$ (sp² hybridization).
   - Structure: Trigonal Planar (no lone pairs).
   - Bond Angle: **120°**.
3. **Analyze NO₂ (Nitrogen Dioxide):**
   - Hybridization: sp² (with one odd electron).
   - Structure: Bent. The single odd electron repels bonding pairs less than a full lone pair but causes deviation.
   - Bond Angle: Approximately **134°**.
4. **Analyze NO₂⁻ (Nitrite Ion):**
   - Hybridization: $H = \frac{1}{2}(5 + 0 - 0 + 1) = 3$ (sp² hybridization).
   - Structure: Bent (one lone pair).
   - Repulsion: Lone pair-bond pair repulsion reduces the angle from 120°.
   - Bond Angle: Approximately **115°**.
5. **Conclusion:** The maximum bond angle is 180° found in NO₂⁺.

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