Iron(III) bromide: Difference between revisions

| Verifiedfields = changed

| verifiedrevid = 432513245

| ImageFile2 = YBr3structure.jpg

| OtherNames = Ferric bromide <br/> Iron tribromide <br/> tribromoiron

|Section1={{Chembox Identifiers

| CASNo_Ref = {{cascite|correct|CAS}}

| CASNo = 10031-26-2

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = 9RDO128EH7

| EINECS = 233-089-1

| PubChem = 25554

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| ChemSpiderID = 23830

| SMILES = [Fe](Br)(Br)Br

| InChI = 1/3BrH.Fe/h3*1H;/q;;;+3/p-3

| InChIKey = FEONEKOZSGPOFN-DFZHHIFOAP

| StdInChI_Ref = {{stdinchicite|correct|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]], [[Pearson symbol|hR24]]

| SpaceGroup = R-3, No. 148

}}

|Section7={{Chembox Hazards

| MainHazards = corrosive

| NFPA-H = 3

| NFPA-F = 0

| NFPA-R = 0

| NFPA-S =

| GHS_ref=<ref>{{cite web |title=C&L Inventory |url=https://echa.europa.eu/information-on-chemicals/cl-inventory-database/-/discli/details/3946 |website=echa.europa.eu}}</ref>

| GHSPictograms = {{GHS07}}

| GHSSignalWord = Warning

| HPhrases = {{H-phrases|315|319|335}}

| PPhrases = {{P-phrases|}}

| FlashPt =

| AutoignitionPt =

'''Iron(III) bromide''' is the [[chemical compound]] with the [[chemical formula|formula]] FeBr₃. Also known as '''ferric bromide''', this red-brown odorless compound is used as a [[Lewis acid]] [[catalyst]] in the [[Electrophilic halogenation|halogenation]] of [[aromatic compounds]]. It dissolves in water to give acidic solutions.

FeBr₃ forms a polymeric structure featuring six-coordinate, [[octahedral]] Fe centers.<ref name=Holleman>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> Although inexpensively available commercially, FeBr₃ can be prepared by treatment of iron metal with [[bromine]]:

Above 200&nbsp;°C, FeBr₃ decomposes to [[Iron(II) bromide|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.

==Uses==

Ferric bromide is occasionally used as an oxidant in [[organic chemistry]], e.g. for the conversion of [[alcohols]] to ketones. It is used as a [[Lewis acid]]ic catalyst for bromination of aromatic compounds. For the latter applications, it is often generated in situ.<ref>{{cite journal|title=Iron(III) bromide|author1=Drapeau, Martin Pichette |author2=Lafantaisie, Mathieu |author3=Ollevier, Thierry |journal=E-EROS Encyclopedia of Reagents for Organic Synthesis|year=2013|doi=10.1002/047084289X.rn01568|isbn=978-0471936237}}</ref>

{{reflist}}

{{bromine compounds}}

[[Category:Iron(III) compounds]]

[[Category:Metal halides]]