Lewis base

Definition

A Lewis base is a chemical species that donates an electron pair to form a covalent bond. It typically has lone pairs of electrons available for donation.

5 Must Know Facts For Your Next Test

1. Lewis bases have lone pairs of electrons that they can donate to Lewis acids.
2. Common examples include ammonia (NH₃), water (H₂O), and hydroxide ions (OH⁻).
3. The strength of a Lewis base depends on the availability of its lone pair electrons.
4. In reactions, Lewis bases often react with Lewis acids to form adducts.
5. Lewis base behavior is crucial in understanding complex formation and catalysis.

Review Questions

• What characteristic allows a molecule to act as a Lewis base?
• Provide two common examples of Lewis bases.
• Explain how the strength of a Lewis base is determined.

Related terms

Lewis acid:

A chemical species that accepts an electron pair to form a covalent bond.

Adduct:

A compound formed from the addition of two or more substances, usually involving a Lewis acid and a Lewis base.

Electron pair donor: Another term for a Lewis base, highlighting its role in donating an electron pair during bond formation.