Lewis

Definition

A Lewis acid is a chemical species that accepts an electron pair, while a Lewis base is a chemical species that donates an electron pair. This concept expands the traditional definitions of acids and bases to include a broader range of chemical reactions.

5 Must Know Facts For Your Next Test

1. Lewis acids are often metal cations or molecules with incomplete octets, such as $AlCl_3$ or $BF_3$.
2. Lewis bases usually have lone pairs of electrons ready for donation, such as $NH_3$ or $H_2O$.
3. The interaction between a Lewis acid and a Lewis base forms a coordinate covalent bond.
4. The strength of Lewis acids and bases can be influenced by the presence of substituents that either withdraw or donate electron density.
5. Lewis acid-base theory can be applied to explain complex formation, catalyst activity, and enzyme function.

Review Questions

Related terms

Coordinate Covalent Bond:

A type of covalent bond in which one atom provides both electrons for the shared pair.

Electrophile: A species that accepts an electron pair during a reaction, often acting as a Lewis acid.

Nucleophile: A species that donates an electron pair during a reaction, often acting as a Lewis base.