Lewis Acid and Lewis Base in Coordination Chemistry

There are various examples of lewis acids and base in coordination chemistry, let’s consider some of these examples in the following reactions:

BF₃ + NH₃ → BF₃:NH₃

In the above reaction boron trifluoride (BF₃) is the Lewis acid because it accepts a pair of electrons from ammonia (NH₃), which acts as the Lewis base. The resulting complex, BF₃:NH₃, is a stable Lewis acid-base complex.

AlCl₃ + CHCl₃ → AlCl₃:CHCl₃

In the above reaction aluminum chloride (AlCl₃) acts as the Lewis acid it accepts a pair of electrons from chloroform (CHCl₃), which acts as the Lewis base. Then formation of the Lewis acid-base complex AlCl₃:CHCl₃.

Cu²⁺ + H₂O → Cu(H₂O)₆²⁺

In the above reaction the copper(II) ion (Cu²⁺) acts as the Lewis acid, and water (H₂O) acts as the Lewis base. Cu²⁺ accepts a pair of electrons from water molecules then forming a complex known as hexaaquacopper(II) ion, [Cu(H₂O)₆]²⁺.

Lewis acids and Lewis bases are main concepts in chemistry, they play a key role in chemical reactions and molecular interactions. These are concepts introduced by Gilbert N. Lewis. These concepts state how the substance interacts and forms new compounds. Lewis acid is a species that accepts electron pairs by creating a bond, whereas Lewis base is a species that donates electron pairs to form bonds with the Lewis acid. This interaction between electron pair donation and acceptance undergoing chemical reactions makes Lewis acids and bases essential tools for molecular behavior and catalysis.

This article explores the differing aspects of these species, specifically, it helps readers to learn about all the significant distinctions between Lewis acids and Lewis bases.