Lewis acid-base theory expands the definition of acids and bases beyond protons, focusing instead on the transfer of electron pairs. A Lewis acid is an electron pair acceptor, while a Lewis base is an electron pair donor, allowing for a broader understanding of chemical reactions and interactions.

Lewis Acid-base Theory

Lewis acid-base theory

definition of acids and bases

transfer of electron pairs

A Lewis acid is a chemical species that can accept an electron pair, making it crucial in forming coordinate covalent bonds. This concept broadens the definition of acids beyond proton donors, allowing for a more comprehensive understanding of acid-base reactions in chemistry.

Lewis acid

An electron pair acceptor is a chemical species that can accept an electron pair from a donor, forming a coordinate covalent bond. This behavior is foundational in Lewis acid-base theory, where electron pair acceptors are classified as Lewis acids.

electron pair acceptor

A Lewis base is a chemical species that donates an electron pair to form a covalent bond, often participating in coordinate covalent bonding with a Lewis acid. This concept is central to understanding acid-base reactions, complex formation, and catalysis in chemistry.

Lewis base

An electron pair donor is a chemical species that provides a pair of electrons to form a covalent bond, often acting as a Lewis base in chemical reactions. This ability to donate electron pairs is fundamental in various chemical processes, including acid-base reactions and coordination chemistry.

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