Chapter 16, Problem 16.2QP

Interpretation Introduction

Interpretation:

For a species to act as Bronsted base, an atom in the species must possess a lone pair of electrons has to be explained.

Concept Introduction: Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  $\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid. Ammonia accepts a proton, and hence it is a Bronsted base.

To Explain: why an atom in species must possess lone pair of electrons, for the species to act as Bronsted base.