" A Lewis acid (named for the American physical chemist Gilbert N. Lewis) 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."
This topic covers the Lewis theory of acids and bases, which defines an acid as an electron acceptor and a base as an electron donor.
Acid-base definitions: Learn the definitions of acids and bases according to the Lewis theory, including how they relate to electron pairs in chemical reactions.
Chemical/Coordinate Bonding: Understand the concept of chemical bonding as it relates to the Lewis theory, especially how coordinate bonding plays an essential role in acid-base reactions.
Lewis Structures: Learn how to write and interpret Lewis structures, including the use of electron-dot diagrams and formal charges.
Electron Pairing and Delocalization: Understand how electron pairing and delocalization affect acid-base reactions, using examples like resonance structures.
Lewis Acid-Base Theory: Learn the Lewis Acid-Base theory and how it describes the interaction between Lewis acids and bases, including examples such as the reaction between a metal cation and a Lewis base.
Hydrogen Ionization Constant: Understand the concept of the hydrogen ionization constant (pKa), and how it relates to acidity and basicity.
Hard-Soft Acid-Base Theory: Explore the concept of hard and soft acids and bases, and how it explains the selectivity observed in many Lewis acid-base reactions.
Ligands: Understand the concept of ligands, how they can act as Lewis bases, and how the strength of the bond between a ligand and a Lewis acid affects the overall acidity/basicity of the Lewis acid.
Applications of Lewis Theory: Investigate the application of Lewis theory in various fields, including biochemistry and coordination chemistry.
Acid-Base Equilibria calculations: Solve acid-base equilibrium problems using Lewis Theory, such as determining the pH of a solution or calculating the equilibrium constant of a reaction.
Lewis Acid-Base Theory: This theory proposes that a molecule can act as a Lewis acid, accepting a pair of electrons, or as a Lewis base, donating a pair of electrons.
Hard-Soft Acid-Base Theory: This theory categorizes acids and bases as "hard" or "soft" based on their relative abilities to accept or donate electrons. "Hard" species are small, highly charged ions and molecules, while "soft" species are larger and more polarizable.
Pearson's Acid-Base Theory: This theory categorizes acids and bases as "soft" or "hard" based on their relative electronegativities and polarizabilities. "Hard" species have high electronegativities and small polarizabilities, while "soft" species have low electronegativities and large polarizabilities.
Lewis-Randall Chemical Potential Equalization Theory: This theory proposes that acid-base reactions occur when the chemical potentials of the reactants are equalized through electron transfer.
Lux-Flood Acid-Base Theory: This theory categorizes acids and bases based on their ability to form hydrogen bonds. "Acidic" species can form strong hydrogen bonds, while "basic" species cannot.
Brønsted-Lowry Acid-Base Theory: This theory defines acids as substances that donate protons and bases as substances that accept protons.
Usanovich Acid-Base Theory: This theory defines acids as substances that are electron-withdrawing and bases as substances that are electron-donating.
Lewis-Basovski Acid-Base Theory: This theory categorizes acids and bases based on their electron-donating or electron-withdrawing capabilities. "Acidic" species are electron-withdrawing, while "basic" species are electron-donating.
Hard-Soft-Medium Theory: This theory categorizes acids and bases as "hard," "soft," or "medium" based on their relative abilities to accept or donate electrons. "Hard" species are small, highly charged ions and molecules, "soft" species are larger and more polarizable, and "medium" species have electronegativities and polarizabilities between those of "hard" and "soft" species.
"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."
"In the context of a specific chemical reaction between NH3 and Me3B, 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."
"The terms nucleophilicity and electrophilicity, emphasize the kinetic aspect of reactivity, while the Lewis basicity and Lewis acidity emphasize the thermodynamic aspect of Lewis adduct formation."
"A Lewis acid is a chemical species that contains an empty orbital."
"A Lewis base is any species that has a filled orbital containing an electron pair which is not involved in bonding."
"Gilbert N. Lewis is an American physical chemist."
"A Lewis base may form a dative bond with a Lewis acid to form a Lewis adduct."
"A Lewis acid is capable of accepting an electron pair from a Lewis base to form a Lewis adduct."
"Gilbert N. Lewis."
"A lone pair of electrons."
"A lone pair."
"An electron pair furnished by the Lewis base."
"The kinetic aspect of reactivity."
"The thermodynamic aspect of Lewis adduct formation."
"Yes, the terms nucleophile and electrophile are more or less interchangeable with Lewis base and Lewis acid, respectively."