Lewis acid-base chemistry

Definition

Lewis acid-base chemistry involves the interaction between Lewis acids (electron pair acceptors) and Lewis bases (electron pair donors). This concept extends the traditional definition of acids and bases to include a broader range of chemical reactions.

5 Must Know Facts For Your Next Test

1. A Lewis acid is any species that can accept an electron pair, such as $\text{BF}_3$ or $\text{AlCl}_3$.
2. A Lewis base is any species that can donate an electron pair, such as $\text{NH}_3$ or $\text{H}_2\text{O}$.
3. Lewis acid-base reactions often result in the formation of a coordinate covalent bond.
4. The strength of a Lewis acid or base depends on its ability to donate or accept electron pairs; for example, metal cations are typically strong Lewis acids.
5. This concept helps explain reactions that do not involve hydrogen ions but still involve electron pair interactions, broadening the types of reactions considered acid-base.

Review Questions

Related terms

Bronsted-Lowry Acid: A substance that donates a proton (H+) in a reaction.

Bronsted-Lowry Base: A substance that accepts a proton (H+) in a reaction.

Coordinate Covalent Bond:

A type of covalent bond where one atom provides both electrons for the bond.