Question

Which of the following molecules has the highest bond angle?

• A. \( \text{CH}_4 \)
• B. \( \text{NH}_3 \)
• C. \( \text{H}_2\text{O} \)
• D. \( \text{BF}_3 \)

Hint:

Bond angle depends on molecular geometry and lone pairs. Fewer lone pairs and planar structures generally lead to larger bond angles.

Answer 1

The Correct Option is D

Step 1: Determine the molecular geometry.

• \( \text{CH}_4 \): Tetrahedral — bond angle \(109.5^\circ\)
• \( \text{NH}_3 \): Trigonal pyramidal — bond angle \(107^\circ\)
• \( \text{H}_2\text{O} \): Bent — bond angle \(104.5^\circ\)
• \( \text{BF}_3 \): Trigonal planar — bond angle \(120^\circ\)

Step 2: Compare bond angles.
Among these, the trigonal planar geometry of \( \text{BF}_3 \) gives the largest bond angle of \(120^\circ\).