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| Names | |
|---|---|
| IUPAC name Iron(III) bromide | |
| Other names Ferric bromide Iron tribromide tribromoiron | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider |
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| ECHA InfoCard | 100.030.069 |
| EC Number |
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| UNII | |
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| Properties | |
| FeBr3 | |
| Molar mass | 295.56 g mol−1 |
| Appearance | brown solid |
| Odor | odorless |
| Density | 4.50 g cm−3 |
| Melting point | 200 °C (392 °F; 473 K) (decomposes) |
| Structure | |
| Trigonal,hR24 | |
| R-3, No. 148 | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | corrosive |
| GHS labelling:[1] | |
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| Warning | |
| H315,H319,H335 | |
| NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Iron(III) bromide is thechemical compound with theformula FeBr3. Also known asferric bromide, this red-brown odorless compound is used as aLewis acidcatalyst in thehalogenation ofaromatic compounds. It dissolves in water to give acidic solutions.
FeBr3 forms a polymeric structure featuring six-coordinate,octahedral Fe centers.[2] Although inexpensively available commercially, FeBr3 can be prepared by treatment of iron metal withbromine:
Above 200 °C, FeBr3 decomposes toferrous bromide:
Iron(III) chloride is considerably more stable, reflecting the greater oxidizing power ofchlorine. FeI3 is not stable, as iron(III) will oxidize iodide ions.
Ferric bromide is occasionally used as an oxidant inorganic chemistry, e.g. for the conversion ofalcohols to ketones. It is used as aLewis acidic catalyst for bromination of aromatic compounds. For the latter applications, it is often generated in situ.[3]
