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

12861 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Why is the first ionisation energy lower in barium compared to calcium?


State and explain how the attraction between nuclei and outermost electrons varies across group 3 (2 marks)


Explain why the first ionisation energy of phosphorous is different to that of sulfur


What is benzene and describe the 2 models used to explain it's structure. Provide a piece of evidence to show which of these models is incorrect.


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences