All Bronsted bases are also Lewis bases but all Bronsted acid are not Lewis acids. Explain.

Explanation

A substance that is capable of giving an electron pair has the tendency to accept a proton e.g.
`H-underset(H)underset(|)overset(H)overset(|)(N)+H-O-H+[H-underset(H)underset(|)overset(H)overset(|)(N)-H]^(+)+OH^(-)`
Here, `NH_(3)` is lewis base as well as Bronsted base. Howver, in a the above case `H_(2)O` is Bronsted acid, because it is giving a proton but is not a lewis acid because it is electronically satisfied.