18.1 Lewis Acids and Bases (Chemistry)
Adduct
A reaction forming only one product
Lewis Acid
(Lone) electron pair acceptor
Lewis Base
(Lone) electron pair donor
Lewis Theory
Acid-base reactions based on electron pair transfer, results in formation of a coordinate covalent bond
Relationship between Bronsted-Lowry and Lewis Theories
All Bronsted Lowry acids are Lewis acids, not all Lewis acids are Bronsted-Lowry acids, Lewis acids do not release H⁺ (same with bases)
Electrophile
An electron-deficient species that accepts a lone pair of electrons from another reactant to form a new covalent bond, lewis acids
Nucleophile
An electron-rich species that donates a lone pair to form a new covalent bond in a reaction, lewis bases
Examples of Electrophiles/Lewis Acids
BF₃, Cu²⁺, Br⁺, NO₂⁺
Lewis Acid-Base Reaction Example (Cu complex)
Cu²⁺ (lewis acid) + 6H₂O (lewis base, ligand) → [Cu(H₂O)₆]²⁺ complex with coordinate bonds
Examples of Nucleophiles/Lewis Bases
HO⁻, NH₃⁺, Cl⁻
