" ... (named for the American physical chemist Gilbert N. Lewis)."
These are bases that can donate an electron pair to an acceptor molecule. Examples include ammonia (NH3), water (H2O), and pyridine (C5H5N).
Bronsted-Lowry acid-base theory: This theory defines an acid as a proton donor and a base as a proton acceptor.
Lewis acid-base theory: This theory defines a Lewis acid as an electron pair acceptor and a Lewis base as an electron pair donor.
Acidic and basic properties of substances: This includes the identification of acidic and basic properties of substances by their pH values, acidity constants, and basicity constants.
Acid and base strength: This includes the concepts of strong and weak acids and bases, and how to identify them through their chemical properties.
Conjugate acid-base pairs: This includes the relationship between acids and their conjugate bases, and bases and their conjugate acids.
Acid-base reactions: This includes the mechanism of acid-base reactions, the equilibrium constant for reactions, and factors that affect the rate of reactions.
Buffer solutions: This includes the concept of buffer solutions, how they work, and how they can be prepared.
Acid-base titrations: This includes the process of acid-base titrations, the selection of an appropriate indicator for a given titration, and the calculation of acid and base concentrations.
Solvent effects: This includes the effect of solvent on acid-base reactions and the dissociation constants of acids and bases.
Lewis structures and electron configuration: This includes the understanding of Lewis structures and electron configuration and its relationship with acid and base properties.
Chemical bonding: This includes the understanding of chemical bonding, and how it relates to the acidity and basicity of substances.
Organic chemistry: This includes the study of organic acids and bases, their chemistry properties, and reactions.
Inorganic chemistry: This includes the study of inorganic acids and bases, their chemical properties, and reactions.
Biochemistry: This includes the study of acid and base reactions in biological systems and how they relate to pH regulation.
Environmental chemistry: This includes the study of acid and base chemistry in the environment, such as acid rain and soil acidity.
Simple Lewis bases: These are molecules or ions that donate a lone pair of electrons to a Lewis acid. They are usually neutral and have a lone pair of electrons on an electronegative atom, such as nitrogen, oxygen, or sulfur.
Anionic Lewis bases: These are ions with a negative charge that donate a lone pair of electrons to a Lewis acid.
Cationic Lewis bases: These are ions with a positive charge that act as donors of electron pairs to Lewis acids.
Chelating Lewis bases: These molecules have two or more donor atoms that bind to the same Lewis acid. The resulting complex is often more stable than a complex with a simple Lewis base.
Bridging Lewis bases: These molecules or ions have two or more donor atoms that can simultaneously bind to two or more Lewis acids, forming a complex with multiple bridging bonds.
Hemilabile Lewis bases: These molecules or ions have donor atoms that can bind to a Lewis acid in one configuration and release the bond in another configuration, allowing for dynamic self-assembly.
Cooperative Lewis bases: These are molecules or ions that have multiple donor atoms that can work together to increase the strength of the donor-acceptor bond.
"A Lewis acid is a chemical species that contains an empty orbital which is capable of accepting an electron pair from a Lewis base to form a Lewis adduct."
"A Lewis base is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a dative bond with a Lewis acid to form a Lewis adduct."
"For example, NH3 is a Lewis base because it can donate its lone pair of electrons."
"Trimethylborane (Me3B) is a Lewis acid as it is capable of accepting a lone pair."
"In a Lewis adduct, the Lewis acid and base share an electron pair furnished by the Lewis base, forming a dative bond."
"A dative bond is formed when a lone pair from NH3 will form a dative bond with the empty orbital of Me3B to form an adduct NH3•BMe3."
"The terms nucleophile and electrophile are more or less interchangeable with Lewis base and Lewis acid, respectively."
"However, these terms, especially their abstract noun forms nucleophilicity and electrophilicity, emphasize the kinetic aspect of reactivity, while the Lewis basicity and Lewis acidity emphasize the thermodynamic aspect of Lewis adduct formation."
"The terminology refers to the contributions of Gilbert N. Lewis."