| 词条 | Iron(III) bromide |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 432513245 | ImageFile = Bismuth-triiodide-layer-3D-balls.png | ImageFile1 = Bismuth-triiodide-layers-stacking-3D-balls.png | ImageFile2 = YBr3structure.jpg | IUPACName = Iron(III) bromide | OtherNames = Ferric bromide Iron tribromide tribromoiron |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|??}} | CASNo = 10031-26-2 | UNII_Ref = {{fdacite|changed|FDA}} | UNII = 9RDO128EH7 | EINECS = | PubChem = 25554 | ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} | ChemSpiderID = 23830 | SMILES = [Fe](Br)(Br)Br | InChI = 1/3BrH.Fe/h3*1H;/q;;;+3/p-3 | InChIKey = FEONEKOZSGPOFN-DFZHHIFOAP | StdInChI_Ref = {{stdinchicite|changed|chemspider}} | StdInChI = 1S/3BrH.Fe/h3*1H;/q;;;+3/p-3 | StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} | StdInChIKey = FEONEKOZSGPOFN-UHFFFAOYSA-K |Section2={{Chembox Properties | Formula = FeBr3 | MolarMass = 295.56 g mol−1 | Appearance = brown solid | Odor = odorless | Density = 4.50 g cm−3 | MeltingPtC = 200 | MeltingPt_notes = (decomposes) | BoilingPt = | Solubility = | LogP = | VaporPressure = | HenryConstant = |Section3={{Chembox Structure | CrystalStruct = Trigonal, hR24 | SpaceGroup = R-3, No. 148 |Section7={{Chembox Hazards | MainHazards = corrosive | NFPA-H = 3 | NFPA-F = 0 | NFPA-R = 0 | NFPA-S = | RPhrases = {{R36/37/38}} | SPhrases = {{S26}} {{S37/39}} | FlashPt = | AutoignitionPt = }} Iron(III) bromide is the chemical compound with the formula FeBr3. Also known as ferric bromide, this red-brown odorless compound is used as a Lewis acid catalyst in the halogenation of aromatic compounds. It dissolves in water to give acidic solutions. Structure, synthesis and basic propertiesFeBr3 forms a polymeric structure featuring six-coordinate, octahedral Fe centers.[1] Although inexpensively available commercially, FeBr3 can be prepared by treatment of iron metal with bromine: 2 Fe + 3 Br2 → 2 FeBr3 Above 200 °C, FeBr3 decomposes to ferrous bromide: 2FeBr3 → 2FeBr2 + Br2 Iron(III) chloride is considerably more stable, reflecting the greater oxidizing power of chlorine. FeI3 is not stable, as iron(III) will oxidize iodide ions. UsesFerric bromide is occasional use as an oxidant in organic chemistry, e.g. for the conversion of alcohols to ketones. It is used as a Lewis acidic catalyst for bromination of aromatic compounds. For the latter applications, it is often generated in situ.[2] See also
References1. ^Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}. {{Iron compounds}}{{bromine compounds}}2. ^{{cite journal|title=Iron(III) bromide|authors=Drapeau, Martin Pichette; Lafantaisie, Mathieu; Ollevier, Thierry|journal=e-EROS Encyclopedia of Reagents for Organic Synthesis|year=2013|doi=10.1002/047084289X.rn01568}} 3 : Iron(Ⅲ) compounds|Bromides|Metal halides |
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