Iron(II) bromide

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Iron(II) bromide
Iron(II) bromide
Names
IUPAC name
Iron(II) bromide
Other names
Ferrous bromide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.244
Properties
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)
soluble
Solubility in other solvents THF, methanol, ethanol
+13,600·10−6 cm3/mol
Structure
Rhombohedral, hP3, SpaceGroup = P-3m1, No. 164
octahedral
Hazards
Main hazards none
R-phrases (outdated) R20 R36/37/38
S-phrases (outdated) S26 S36
Related compounds
Other anions
Iron(II) chloride
Other cations
iron(III) bromide
Related compounds
VBr2
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Iron(II) bromide is the chemical compound with the chemical formula FeBr2. The anhydrous compound is a yellow or brownish-colored paramagnetic solid. It is a common precursor to other iron compounds in research laboratory. Several hydrates of FeBr2 are also known.

Structure[edit]

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.

Synthesis and reactions[edit]

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.[2] Iron(II) bromide cannot be formed by the reaction of iron and bromine, because that reaction would produce ferric bromide.[citation needed]

FeBr2 reacts with 2 equivalents of (C2H5)4NBr to give [(C2H5)4N]2FeBr4.[3]

FeBr2 reacts with bromide and bromine to form the intensely colored, mixed-valence species [FeBr3Br9].[4]

FeBr2 is a weak reducing agent, as are all ferrous compounds.[citation needed]

References[edit]

  1. ^ Haberecht, J.; Borrmann, H.; Kniep, R. "Refinement of the Crystal Structure of Iron Dibromide, FeBr2" Zeitschrift für Kristallographie - New Crystal Structures 2001, vol. 216, p. 510. doi:10.1524/ncrs.2001.216.14.544
  2. ^ G. Winter, "Iron(II) Halides" "Inorganic Syntheses" 1973, volume 14, pages 101-104. doi: 10.1002/9780470132456.ch20
  3. ^ N. S. Gill, F.. B. Taylor Inorganic Syntheses 1967, volume 9, page 136-142. doi: 10.1002/9780470132401.ch37
  4. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5