What is the Difference Between Bronsted and Lewis?

The main difference between Bronsted-Lowry and Lewis acids and bases lies in their definitions and the components they involve. Here is a comparison of the two theories:

Bronsted-Lowry Acids and Bases:

1. A Bronsted-Lowry acid is a compound that can donate a hydrogen ion (H+ or proton).
2. A Bronsted-Lowry base is a compound that can accept a hydrogen ion.

Lewis Acids and Bases:

1. A Lewis acid is a compound that can accept a pair of electrons.
2. A Lewis base is a compound that can donate a pair of electrons.

In summary, Bronsted-Lowry acids and bases focus on the transfer of hydrogen ions (protons), while Lewis acids and bases focus on the transfer of electron pairs. These two theories can sometimes overlap, as some substances can act as both Bronsted-Lowry and Lewis acids or bases, depending on the reaction.

Comparative Table: Bronsted vs Lewis

The main difference between Brønsted-Lowry and Lewis acid-base definitions lies in their focus on proton transfer versus electron transfer. Here is a comparison table highlighting the differences:

A Brønsted-Lowry acid is a substance that donates a proton (H+) in a chemical reaction, while a Brønsted-Lowry base is a substance that accepts a proton (H+) in a chemical reaction. On the other hand, a Lewis acid is a substance that accepts an electron pair, and a Lewis base is a substance that donates an electron pair in a chemical reaction.