Iron(II) bromide

Names
IUPAC name

Iron(II) bromide

Other names

Ferrous bromide

Identifiers

CAS Number

* 20049-61-0 tetrahydrate
* 7789-46-0 anhydrous

3D model (JSmol)

* Interactive image

ChemSpider |

* 74218 Y

PubChem CID

* 425646

UNII |

* EA3X054RBZ Y

InChI

* InChI=1S/2BrH.Fe/h2*1H;/q;;+2/p-2 Y

Key: GYCHYNMREWYSKH-UHFFFAOYSA-L Y

* InChI=1/2BrH.Fe/h2*1H;/q;;+2/p-2

Key: GYCHYNMREWYSKH-NUQVWONBAN

SMILES

* [Fe+2].[Br-].[Br-]

Properties

Chemical formula

| FeBr2
Molar mass | 215.65 g mol−1
Appearance  | yellow-brown solid
Density | 4.63 g cm−3, solid
Melting point |  684 °C (1,263 °F; 957 K) (anhydrous)
27 °C (Hexahydrate)
Boiling point |  934 °C (1,713 °F; 1,207 K)

Solubility in water

| 117 g / 100 ml
Solubility in other solvents  | THF, methanol, ethanol

Magnetic susceptibility (χ)

| +13,600·10−6 cm3/mol
Structure

Crystal structure

| Rhombohedral, hP3, SpaceGroup = P-3m1, No. 164

Coordination geometry

| octahedral
Hazards
Main hazards | none
Related compounds

Other anions

| Iron(II) fluoride
Iron(II) chloride
Iron(II) iodide

Other cations

| Manganese(II) bromide
Cobalt(II) bromide

Related compounds

| Vanadium(II) bromide
Iron(III) bromide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Iron(II) bromideIron(II) bromide anhydrous

Iron(II) bromide refers to inorganic compounds with the chemical formula FeBr2(H2O)x. The anhydrous compound (x = 0) is a yellow or brownish-colored paramagnetic solid. The tetrahydrate is also known, all being pale colored solids. They are common precursor to other iron compounds.

## Contents

* 1 Structure
* 2 Synthesis and reactions
* 3 Magnetism
* 4 References

## Structure

Like most metal halides, FeBr2 adopts a polymeric structure consisting of isolated metal centers cross-linked with halides. It crystallizes with the CdI2 structure, featuring close-packed layers of bromide ions, between which are located Fe(II) ions in octahedral holes.[1] The packing of the halides is slightly different from that for FeCl2, which adopts the CdCl2 motif. The tetrahydrates FeX2(H2O)4 (X = Cl, Br) have similar structures, with octahedral metal centers and mutually trans halides.[2]

## Synthesis and reactions

FeBr2 is synthesized using a methanol solution of concentrated hydrobromic acid and iron powder. It adds the methanol solvate [Fe(MeOH)6]Br2 together with hydrogen gas. Heating the methanol complex in a vacuum gives pure FeBr2.[3]

FeBr2 reacts with two equivalents of tetraethylammonium bromide to give [(C2H5)4N]2FeBr4.[4] FeBr2 reacts with bromide and bromine to form the intensely colored, mixed-valence species [FeBr3Br9]−.[5]

## Magnetism

FeBr2 possesses a strong metamagnetism at 4.2 K and has long been studied as a prototypical metamagnetic compound.[6][7]

## References

1. ↑ Haberecht, J.; Borrmann, Η.; Kniep, R. (2001). "Refinement of the crystal structure of iron dibromide, FeBr2". Zeitschrift für Kristallographie - New Crystal Structures 216 (1–4). doi:10.1524/ncrs.2001.216.14.544.
2. ↑ Waizumi, Kenji; Masuda, Hideki; Ohtaki, Hitoshi (1992). "X-ray Structural Studies of FeBr2·4H2O, CoBr2·4H2O, NiCl2·4H2O and CuBr2·4H2O. Cis/Trans Selectivity in Transition Metal(II) Dihalide Tetrahydrate". Inorganica Chimica Acta 192 (2): 173–181. doi:10.1016/S0020-1693(00)80756-2.
3. ↑ Winter, G. (1973). "Iron(II) Halides". Inorganic Syntheses. Inorganic Syntheses. 14. pp. 99–104. doi:10.1002/9780470132456.ch20. ISBN 9780470132456.
4. ↑ N. S. Gill, F.. B. Taylor Inorganic Syntheses 1967, volume 9, page 136-142. doi: 10.1002/9780470132401.ch37
5. ↑ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5
6. ↑ Wilkinson, M. K.; Cable, J. W.; Wollan, E. O.; Koehler, W. C. (15 January 1959). "Neutron Diffraction Investigations of the Magnetic Ordering in FeBr2, CoBr2, FeCl2, and CoCl2". Physical Review 113 (2): 497–507. doi:10.1103/PhysRev.113.497. Bibcode: 1959PhRv..113..497W.
7. ↑ Jacobs, I. S.; Lawrence, P. E. (10 December 1967). "Metamagnetic Phase Transitions and Hysteresis in FeCl2". Physical Review 164 (2): 866–878. doi:10.1103/PhysRev.164.866. Bibcode: 1967PhRv..164..866J.

* v
* t
* e

Iron compounds

Fe(-II)|

* Na2Fe(CO)4

Fe(0)|

* Fe(CO)5
* Fe2(CO)9
* Fe3(CO)12
* Fe(CO)3CH3COC2H2C6H6

Fe(I)|

* FeH

| Organoiron(I) compounds|

* (C5H5FeCO)2(CO)2

|

Fe(0,II)|

* Fe3C

Fe(II)|

* FeBr2
* FeCl2
* FeF2
* FeI2
* FeH2
* FeMoO4
* FeO
* Fe(OH)2
* FeS
* FeSO4
* FeSe
* FeSeO4
* FeSi2
* FeTiO3
* FeCO3
* FeC2O4
* Fe(C2H3O2)2
* Fe(C3H5O3)2
* FeC6H6O7
* FeC12H22O14
* Fe2CrO4
* Fe3(PO4)2
* H2Fe(CO)4
* Fe(HCO3)2
* Mg2FeH6

| Organoiron(II) compounds|

* Fe(C5H5)2
* Fe(C5H4P(C6H5)2)2
* C4H4Fe(CO)3
* C4H6Fe(CO)3

|

Fe(0,III)|

* Fe3P

Fe(II,III)|

* Fe3O4
* Fe3S4

Fe(III)|

* FeBr3
* FeCl3
* FeF3
* FeI3
* Fe(NO3)3
* Fe(acac)3
* FeOCl
* FeO(OH)
* FePO4
* Fe4(P2O7)3
* Fe2(CrO4)3
* Fe2(C2O4)3
* Fe2O3
* Fe2S3
* Fe2(SO4)3
* FeBO3
* FeB

| Organoiron(III) compounds|

* Fe(C5H5)2BF4
* C6H8O7⋅xFe3+⋅yNH3

|

Fe(VI)|

* K2FeO4
* BaFeO4

* v
* t
* e

Bromine compounds

* AgBr
* AlBr3
* AmBr3
* AsBr3
* AuBr3
* BBr3
* B2Br4
* BaBr2
* BeBr2
* BiBr3
* BrCl
* CsBr
* BrF3
* BrF5
* HBr
* IBr
* KBr
* LiBr
* BrN3
* NaBr
* BrO2
* RbBr
* TlBr
* CaBr2
* CdBr2
* CoBr2
* CuBr2
* EuBr2
* FeBr2
* GeBr2
* HgBr2
* Hg2Br2
* MgBr2
* MnBr2
* NiBr2
* Br2O
* Br2O3
* Br2O5
* PbBr2
* PdBr2
* PtBr2
* RaBr2
* S2Br2
* Se2Br2
* SnBr2
* SrBr2
* TeBr2
* YbBr2
* ZnBr2
* CeBr3
* CrBr3
* CsBr3
* DyBr3
* ErBr3
* EuBr3
* FeBr3
* GaBr3
* GdBr3
* HoBr3
* InBr
* InBr3
* IrBr3
* LaBr3
* LuBr3
* MoBr3
* NBr3
* NdBr3
* PBr3
* PrBr3
* ReBr3
* SbBr3
* SmBr3
* TbBr3
* TmBr3
* UBr3
* VBr3
* YBr3
* YbBr3
* GeBr4
* HfBr4
* PbBr4
* SeBr4
* SiBr4
* SnBr4
* TeBr4
* ThBr4
* TiBr4
* UBr4
* WBr4
* ZrBr4
* NbBr5
* PBr5
* TaBr5
* UBr5
* WBr5
* CBr4
* CrBr2
* DyBr2
* HfBr2
* HfBr3

Chemical formulas

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