18.1 Lewis Acids and Bases (Chemistry)

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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⁻


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