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NEET CHEMISTRYChemical Bonding and Molecular StructureMedium

Question

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⁺.

Exam Context & Concepts Covered

This question aligns with the NEET CHEMISTRY syllabus, specifically targeting concepts from Chemical Bonding and Molecular Structure. Mastering this topic is crucial for scoring well in the upcoming medical entrance examinations. Solving conceptually related problems will help you understand the nuances of these concepts and improve your problem-solving speed.

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