Why is the bond angle in an amide ion smaller than the bond angle in a molecule of ammonia?

The nitrogen atom in both NH3 and NH2- has 8 outer shell electrons. In NH3, 3 pairs of these electrons are used in covalent bonding to hydrogen atoms and the remaining 2 electrons exist as a lone pair. In NH2, there are 2 lone pairs of electrons due to there only being 2 hydrogen atoms involved in covalent bonding. Lone pairs create a stronger repulsion than bonding pairs. This results in a smaller bond angle in the amide ion due to the increased repulsion due to the extra lone pair. The repulsive force pushes the covalent bonds closer together.

Answered by Anna G. Chemistry tutor

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