Iron(II) bromide: Difference between revisions
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{{chembox |
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| Name = Iron(II) bromide |
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| ImageFile1 =FeBr2(aq)4.svg |
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| ImageFile2 = Cadmium-iodide-3D-layers.png |
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| ImageName = Iron(II) bromide |
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| IUPACName = Iron(II) bromide |
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| SystematicName = |
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| Section1 = {{Chembox Identifiers |
| Section1 = {{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 74218 |
| ChemSpiderID = 74218 |
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| InChI = 1/2BrH.Fe/h2*1H;/q;;+2/p-2 |
| InChI = 1/2BrH.Fe/h2*1H;/q;;+2/p-2 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = GYCHYNMREWYSKH-UHFFFAOYSA-L |
| StdInChIKey = GYCHYNMREWYSKH-UHFFFAOYSA-L |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo1 = 20049-61-0 |
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| CASNo1_Comment= tetrahydrate |
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| CASNo2_Comment= anhydrous |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = EA3X054RBZ |
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| PubChem = 425646 |
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| Section2 = {{Chembox Properties |
| Section2 = {{Chembox Properties |
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| Formula = FeBr<sub>2</sub> |
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| MolarMass = 215.65 g mol<sup>−1</sup> |
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| Appearance = yellow-brown solid |
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| Density = 4.63 g cm<sup>−3</sup>, solid |
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| Solubility = 117 g / 100 ml |
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| Solvent = other solvents |
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| SolubleOther = [[THF]], [[methanol]], [[ethanol]] |
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| MeltingPtC = 684 |
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| MeltingPt_notes = (anhydrous) <br> 27 °C (Hexahydrate) |
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| BoilingPtC = 934 |
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| MagSus = +13,600·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section3 = {{Chembox Structure |
| Section3 = {{Chembox Structure |
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| Coordination = octahedral |
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| CrystalStruct = [[Rhombohedral]], [[Pearson symbol|hP3]], SpaceGroup = P-3m1, No. 164 |
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| Dipole = |
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| Section7 = {{Chembox Hazards |
| Section7 = {{Chembox Hazards |
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| ExternalSDS = |
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| MainHazards = none |
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| FlashPt = |
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| RPhrases = {{R20}} {{R36/37/38}} |
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| SPhrases = {{S26}} {{S36}} |
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| Section8 = {{Chembox Related |
| Section8 = {{Chembox Related |
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| OtherAnions = [[Iron(II) fluoride]]<br>[[Iron(II) chloride]]<br>[[Iron(II) iodide]] |
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| OtherCations = [[Manganese(II) bromide]]<br>[[Cobalt(II) bromide]] |
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| OtherFunction_label = compounds |
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| OtherFunction = [[Vanadium(II) bromide]]<br>[[Iron(III) bromide]] |
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| OtherFunctn = VBr<sub>2</sub> |
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[[File:Бромид железа.jpg|alt=Iron(II) bromide|thumb|Iron(II) bromide anhydrous]] |
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'''Iron(II) bromide''' |
'''Iron(II) bromide''' refers to [[inorganic compound]]s with the chemical formula FeBr<sub>2</sub>(H<sub>2</sub>O)<sub>x</sub>. The anhydrous compound (x = 0) is a yellow or brownish-colored paramagnetic solid. The [[water of crystallization|tetrahydrate]] is also known, all being pale colored solids. They are common precursor to other iron compounds. |
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==Structure== |
==Structure== |
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Like most metal halides, FeBr<sub>2</sub> adopts a polymeric structure consisting of isolated metal centers cross-linked with halides. |
Like most metal halides, FeBr<sub>2</sub> adopts a polymeric structure consisting of isolated metal centers cross-linked with halides. It crystallizes with the CdI<sub>2</sub> structure, featuring close-packed layers of bromide ions, between which are located Fe(II) ions in octahedral holes.<ref>{{cite journal|doi=10.1524/ncrs.2001.216.14.544|title=Refinement of the crystal structure of iron dibromide, FeBr2|journal=Zeitschrift für Kristallographie - New Crystal Structures|volume=216|issue=1–4|year=2001|last1=Haberecht|first1=J.|last2=Borrmann|first2=Η.|last3=Kniep|first3=R.|doi-access=free}}</ref> The packing of the halides is slightly different from that for FeCl<sub>2</sub>, which adopts the CdCl<sub>2</sub> motif. The tetrahydrates FeX<sub>2</sub>(H<sub>2</sub>O)<sub>4</sub> (X = Cl, Br) have similar structures, with octahedral metal centers and mutually trans halides.<ref>{{cite journal |doi=10.1016/S0020-1693(00)80756-2| title=X-ray Structural Studies of FeBr<sub>2</sub>·4H<sub>2</sub>O, CoBr<sub>2</sub>·4H<sub>2</sub>O, NiCl<sub>2</sub>·4H<sub>2</sub>O and CuBr<sub>2</sub>·4H<sub>2</sub>O. Cis/Trans Selectivity in Transition Metal(II) Dihalide Tetrahydrate | year=1992 | last1=Waizumi | first1=Kenji | last2=Masuda | first2=Hideki | last3=Ohtaki | first3=Hitoshi | journal=Inorganica Chimica Acta | volume=192 | issue=2 | pages=173–181 }}</ref> |
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==Synthesis== |
==Synthesis and reactions== |
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FeBr<sub>2</sub> is |
FeBr<sub>2</sub> is synthesized using a [[methanol]] solution of concentrated [[hydrobromic acid]] and iron powder. It adds the methanol solvate [Fe(MeOH)<sub>6</sub>]Br<sub>2</sub> together with hydrogen gas. Heating the methanol complex in a vacuum gives pure FeBr<sub>2</sub>.<ref>{{cite book|doi=10.1002/9780470132456.ch20|chapter=Iron(II) Halides|series=Inorganic Syntheses|pages=99–104|year=1973|volume=14| last1=Winter|first1=G.|title=Inorganic Syntheses|isbn=9780470132456}}</ref> |
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⚫ | FeBr<sub>2</sub> reacts with two equivalents of [[tetraethylammonium bromide]] to give [(C<sub>2</sub>H<sub>5</sub>)<sub>4</sub>N]<sub>2</sub>FeBr<sub>4</sub>.<ref>N. S. Gill, F.. B. Taylor Inorganic Syntheses 1967, volume 9, page 136-142. {{doi| 10.1002/9780470132401.ch37}}</ref> FeBr<sub>2</sub> reacts with bromide and bromine to form the intensely colored, mixed-valence species [FeBr<sub>3</sub>Br<sub>9</sub>]<sup>−</sup>.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}</ref> |
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Iron(II) bromide cannot be formed by the reaction of [[iron]] and [[bromine]], because that reaction would produce [[ferric bromide]]. |
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==Magnetism== |
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FeBr<sub>2</sub> possesses a strong [[metamagnetism]] at 4.2 [[Kelvin|K]] and has long been studied as a prototypical metamagnetic compound.<ref>{{cite journal |last1=Wilkinson |first1=M. K. |last2=Cable |first2=J. W. |last3=Wollan |first3=E. O. |last4=Koehler |first4=W. C. |title=Neutron Diffraction Investigations of the Magnetic Ordering in FeBr<sub>2</sub>, CoBr<sub>2</sub>, FeCl<sub>2</sub>, and CoCl<sub>2</sub> |journal=Physical Review |date=15 January 1959 |volume=113 |issue=2 |pages=497–507 |doi=10.1103/PhysRev.113.497|bibcode=1959PhRv..113..497W }}</ref><ref>{{cite journal |last1=Jacobs |first1=I. S. |last2=Lawrence |first2=P. E. |title=Metamagnetic Phase Transitions and Hysteresis in FeCl<sub>2</sub> |journal=Physical Review |date=10 December 1967 |volume=164 |issue=2 |pages=866–878 |doi=10.1103/PhysRev.164.866|bibcode=1967PhRv..164..866J }}</ref> |
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FeBr<sub>2</sub> reacts with (C<sub>2</sub>H<sub>5</sub>)<sub>4</sub>NBr to give [(C<sub>2</sub>H<sub>5</sub>)<sub>4</sub>N]<sub>2</sub>FeBr<sub>4</sub>.<ref>N. S. Gill, F.. B. Taylor Inorganic Syntheses 1967, volume 9, page 136-142.</ref> |
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FeBr<sub>2</sub> is a weak reducing agent, as are all [[ferrous]] compounds. |
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==References== |
==References== |
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<references/> |
<references/> |
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{{Iron compounds}} |
{{Iron compounds}} |
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{{bromine compounds}} |
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[[Category:Bromides]] |
[[Category:Bromides]] |
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[[Category: |
[[Category:Iron(II) compounds]] |
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[[Category:Iron compounds]] |
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[[Category:Metal halides]] |
[[Category:Metal halides]] |
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{{inorganic-compound-stub}} |
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[[ar:بروميد الحديد الثنائي]] |
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[[de:Eisen(II)-bromid]] |
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[[nl:IJzer(II)bromide]] |
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[[zh:溴化亚铁]] |