Question

.Which of the following describes the property of ammonia that allows it to function as a Brønsted base and a Lewis base?

a) Its ability to accept a proton and donate electron pairs
b) Its capacity to donate a proton and accept electron pairs
c) Its inert nature in chemical reactions
d) Its inability to form bonds with other molecules

Answer 1

Ammonia showcases its dual functionality as a Brønsted base by accepting protons, and as a Lewis base by donating electron pairs to form covalent bonds with Lewis acids.

Step-by-step explanation:

The property of ammonia that allows it to function as a Brønsted base and a Lewis base is its ability to accept a proton and to donate electron pairs.

As a Brønsted base, ammonia (NH3) can accept a proton from another molecule such as water (H2O), which makes water the Brønsted-Lowry acid.

In this process, a hydrogen ion (H+) is transferred to the ammonia, forming ammonium ion (NH4+). As a Lewis base, ammonia can donate a pair of electrons to form a covalent bond, particularly with compounds that can accept electron pairs, thereby acting as Lewis acids.

An example would be the reaction between ammonia and a silver ion (Ag+), where the nitrogen atom in ammonia donates its lone pair to form a bond with the silver ion.