Chapter 16, Problem 16.117QP

Interpretation Introduction

Interpretation:

All Bronsted acids are Lewis acids, but the reverse is not true has to be explained with two examples

Concept Information:

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.

According to Lewis theory, acid and base can be defined as follows.

Lewis Acid:

Lewis acid is a substance that can accept a pair of electrons

Example: $\text{BF}{\text{3}}_{}$

Lewis Base:

Lewis base is a substance that can donate a pair of electrons.

Example: ${\text{NH}}_{\text{3}}$

To explain: All Bronsted acids are Lewis acids, but the reverse is not true.