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

To determine which molecule has the highest bond angle, we need to consider their molecular geometries:

• \( \text{CH}_4 \): Methane is a tetrahedral molecule with bond angles of \(109.5^\circ\).
• \( \text{NH}_3 \): Ammonia has a trigonal pyramidal shape due to the lone pair on nitrogen, resulting in bond angles of approximately \(107^\circ\).
• \( \text{H}_2\text{O} \): Water has a bent shape with two lone pairs, causing bond angles of about \(104.5^\circ\).
• \( \text{CO}_2 \): Carbon dioxide is a linear molecule with bond angles of \(180^\circ\).

Among these molecules, \( \text{CO}_2 \) has the highest bond angle, which is \(180^\circ\).

Answer 2

To determine which molecule has the highest bond angle, we must consider the molecular geometry of each molecule:

• \( \text{CH}_4 \): Methane has a tetrahedral geometry with bond angles of approximately \(109.5^\circ\).
• \( \text{NH}_3 \): Ammonia has a trigonal pyramidal shape. The lone pair on the nitrogen atom compresses the bond angles slightly to about \(107^\circ\).
• \( \text{H}_2\text{O} \): Water has a bent shape with two lone pairs causing bond angles to decrease to approximately \(104.5^\circ\).
• \( \text{CO}_2 \): Carbon dioxide is linear with bond angles of \(180^\circ\).

Based on these geometries, \( \text{CO}_2 \) has the highest bond angle of \(180^\circ\).