Lewis bases
Lewis Bases
A Lewis base is a chemical species that donates an electron pair to form a chemical bond in a reaction. This concept was first proposed by Gilbert N. Lewis in 1923, and it forms a significant part of the Lewis theory of acids and bases. Lewis bases are also known as electron-pair donors.
Characteristics[edit | edit source]
Lewis bases are characterized by their ability to donate a pair of electrons to a Lewis acid during a chemical reaction. This electron-pair donation results in the formation of a coordinate covalent bond, also known as a dative bond. The strength of a Lewis base is determined by its ability to donate electrons, which is influenced by factors such as the base's polarity, electronegativity, and the presence of lone pairs of electrons.
Examples[edit | edit source]
Common examples of Lewis bases include water (H2O), ammonia (NH3), and hydroxide ion (OH-). These substances can donate a pair of electrons to a Lewis acid to form a coordinate covalent bond.
Applications[edit | edit source]
Lewis bases have wide-ranging applications in chemistry, particularly in catalysis, organic synthesis, and coordination chemistry. They are used in the formation of complexes with metals, in polymerization reactions, and in the synthesis of various organic compounds.
See also[edit | edit source]
References[edit | edit source]
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Contributors: Prab R. Tumpati, MD
