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NEET CHEMISTRYMedium

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

A

NO₂

B

NO₂⁻

C

NO₂⁺

D

NO₃⁻

Step-by-Step Solution

  1. Analyze NO₂⁺ (Nitronium Ion):
  • Hybridization: H=12(V+M−C+A)=12(5+0−1+0)=2H = \frac{1}{2}(V + M - C + A) = \frac{1}{2}(5 + 0 - 1 + 0) = 2 (sp hybridization).
  • Structure: Linear.
  • Bond Angle: 180°.
  1. Analyze NO₃⁻ (Nitrate Ion):
  • Hybridization: H=12(5+0−0+1)=3H = \frac{1}{2}(5 + 0 - 0 + 1) = 3 (sp² hybridization).
  • Structure: Trigonal Planar (no lone pairs).
  • Bond Angle: 120°.
  1. 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°.
  1. Analyze NO₂⁻ (Nitrite Ion):
  • Hybridization: H=12(5+0−0+1)=3H = \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°.
  1. Conclusion: The maximum bond angle is 180° found in NO₂⁺.
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