KnowraLewis acidLinked fromLinked fromThe 48 pages that link to Lewis acid, each with the reason it gives.All 48Broader topic 1Related 17Narrower topic 24Compared with 6ElectrophileNarrower topic: Electrophiles are Lewis acids when they accept electron pairs during bond formation.Hard and soft acids and basesNarrower topic: HSAB applies its hardness and softness categories to electron-pair acceptors.Friedel–Crafts reactionNarrower topic: Lewis acids such as aluminum chloride activate reagents by accepting electron pairs.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.Boric acidNarrower topic: Boric acid accepts a hydroxide ion’s electron pair rather than donating a proton directly.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.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.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.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.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.Solid acidNarrower topic: Lewis-acid sites accept electron pairs from reactants bound at the solid surface.
KnowraLewis acidLinked fromLinked fromThe 48 pages that link to Lewis acid, each with the reason it gives.All 48Broader topic 1Related 17Narrower topic 24Compared with 6ElectrophileNarrower topic: Electrophiles are Lewis acids when they accept electron pairs during bond formation.Hard and soft acids and basesNarrower topic: HSAB applies its hardness and softness categories to electron-pair acceptors.Friedel–Crafts reactionNarrower topic: Lewis acids such as aluminum chloride activate reagents by accepting electron pairs.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.Boric acidNarrower topic: Boric acid accepts a hydroxide ion’s electron pair rather than donating a proton directly.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.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.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.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.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.Solid acidNarrower topic: Lewis-acid sites accept electron pairs from reactants bound at the solid surface.