Basicity of Amines - Practice Questions & MCQ

Amines like ammonia are basic in nature. The basic nature is due to the presence of an unshared pair of electrons on nitrogen atom. This lone pair of electrons is available for the formation of a new bond with a proton or Lewis acids.

Amines are weak bases as they combine partially with the water to form hydroxyl ions.

Alkylamines are stronger bases than ammonia. This can be explained in terms of electron releasing inductive effect of alkyl group. As a result, the electron density on the nitrogen atom increases and thus, they can donate the lone pair of electrons more easily than ammonia.

The electron releasing effect is maximum in tertiary amines and minimum in primary amines.
3^o Amine > 2^o Amine > 1^o Amine > NH₃
However, the actual order of basicity in the case of lower members is found to be as:
2^o Amine > 1^o Amine > 3^o Amine > NH₃