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. \( \text{CO}_2 \)

Hint:

Remember: Lone pairs reduce bond angles. Linear structures like CO\(_2\) have the maximum angle.

Answer 1

The Correct Option is D

The bond angle is determined by molecular geometry:

• \( \text{CH}_4 \): Tetrahedral, \(109.5^\circ\) bond angles.
• \( \text{NH}_3 \): Trigonal pyramidal due to a lone pair on nitrogen, approximately \(107^\circ\) bond angles.
• \( \text{H}_2\text{O} \): Bent shape with two lone pairs, approximately \(104.5^\circ\) bond angles.
• \( \text{CO}_2 \): Linear, \(180^\circ\) bond angles.

The highest bond angle among these molecules is \(180^\circ\), found in \( \text{CO}_2 \).