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.

• ElectrophileNarrower topic: Electrophiles are Lewis acids when they accept electron pairs during bond formation.

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

• pKaCompared with: Lewis acidity concerns electron-pair acceptance, not necessarily proton dissociation measured by pKa.

• Conjugate acidCompared with: Lewis acidity does not require the proton transfer that defines conjugate acids here.

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

• Hard and soft acids and basesNarrower topic: HSAB applies its hardness and softness categories to electron-pair acceptors.

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

• Friedel–Crafts reactionNarrower topic: Lewis acids such as aluminum chloride activate reagents by accepting electron pairs.

• OxoacidCompared with: This broader acid definition does not require proton donation, unlike oxoacid behavior in Brønsted terms.

• SuperacidCompared with: Some superacids combine proton donation with strong Lewis-acid behavior.

• Brønsted–Lowry acidNarrower topic: The Lewis definition includes proton acceptors and other electron-pair acceptors.

• Friedel–Crafts acylationNarrower topic: Lewis acids activate acyl halides and influence the reaction’s required conditions.

• Hydrogen ionCompared with: A Lewis acid need not be a hydrogen ion or donate a proton.

• Boric acidNarrower topic: Boric acid accepts a hydroxide ion’s electron pair rather than donating a proton directly.

• Gilbert N. LewisBroader topic: Lewis broadened acid chemistry beyond proton transfer with this electron-pair definition.

• 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.

• Acid strengthCompared with: Lewis acidity is defined by electron-pair acceptance, not proton donation.

• BorateNarrower topic: Boric acid accepts hydroxide’s electron pair as aqueous borate forms.

• BrominationNarrower topic: Lewis acids such as FeBr₃ activate Br₂ for aromatic bromination.

• 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.

• Iron(III) chlorideNarrower topic: Iron(III) chloride accepts electron pairs from substrates in reactions such as aromatic chlorination.

• Phosphorus pentachlorideNarrower topic: PCl₅ can accept electron pairs and form complexes such as [PCl₆]⁻.

• Aluminium chlorideNarrower topic: AlCl₃ accepts electron pairs, accounting for its role in many catalytic reactions.

• Antimony pentafluorideNarrower topic: SbF₅ accepts fluoride and other electron pairs, making it a particularly strong example.

• Fluoroantimonic acidNarrower topic: Antimony pentafluoride’s Lewis acidity drives the mixture’s strong proton-donating behavior.

• Magic acidNarrower topic: Antimony pentafluoride boosts magic acid's strength by acting as a Lewis acid.

• Boron trifluorideNarrower topic: BF₃ accepts electron pairs, the defining behavior that underlies its catalytic action.

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

• Zinc chlorideNarrower topic: Zinc chloride accepts electron pairs, accounting for its catalytic action in many reactions.

• Aluminium fluorideNarrower topic: Aluminium centers in fluoride compounds can accept electron pairs from coordinating ligands.

• 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.

• Titanium tetrachlorideNarrower topic: TiCl₄ accepts electron pairs, accounting for its catalytic behavior in many reactions.

• Antimony trichlorideNarrower topic: SbCl₃ accepts electron pairs, accounting for much of its reactivity.

• Beryllium chlorideNarrower topic: Electron-pair acceptance explains why BeCl₂ forms complexes with donor molecules.

• 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.

• HSAB theoryNarrower topic: HSAB classifies Lewis acids by how concentrated or deformable their charge is.

• Phosphoryl chlorideNarrower topic: POCl₃ accepts electron density at phosphorus during many activation reactions.

• Tin(IV) chlorideNarrower topic: Tin(IV) chloride accepts electron pairs from bases and donor molecules.

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

• Solid acidNarrower topic: Lewis-acid sites accept electron pairs from reactants bound at the solid surface.

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