Linked from

The 48 pages that link to Lewis acid, each with the reason it gives.

• ChelationRelated: Metal ions accept electron pairs from the donor atoms of chelating molecules.

• Formal chargeRelated: Changes in formal charge can track electron-pair donation during Lewis acid–base reactions.

• Nucleophilic additionRelated: Lewis acids can activate an electrophilic multiple bond toward nucleophilic attack.

• AluminaRelated: Exposed aluminum sites on alumina surfaces can act as Lewis acid sites.

• AcidityRelated: The Lewis definition extends acidity beyond proton transfer.

• Lewis baseRelated: It receives the pair donated by a Lewis base, completing the defining interaction.

• Cationic polymerizationRelated: Lewis acids often activate initiators or monomers to generate cationic centers.

• Sodium borohydrideRelated: Lewis acids can activate borohydride reagents or alter their reducing behavior.

• Magnesium ionRelated: Mg²⁺ accepts electron pairs from ligands, helping explain its attraction to oxygen atoms.

• Electron-deficient compoundRelated: Many electron-deficient compounds accept donor pairs, though electron deficiency and Lewis acidity are not identical.

• Organic acidRelated: Some organic acids act as electron-pair acceptors without donating a proton.

• Boron groupRelated: Electron-poor boron compounds readily accept electron pairs.

• Tin(II) chlorideRelated: Tin(II) centers can accept electron pairs from ligands, contributing to complex formation.

• Boron trioxideRelated: Boron centers in B₂O₃ can accept electron density from oxygen-containing species.

• Electrophilic substitutionRelated: Lewis acids often generate or strengthen the electrophile used in substitution.

• Aluminium nitrateRelated: Aluminium ions accept electron pairs from water molecules in solution.

• Zinc iodideRelated: Zinc iodide can coordinate to electron-rich groups and activate reactants.