7789-46-0

Basic information

• Product Name: IRON (II) BROMIDE
• Synonyms: FeBr2;Iron bromide (FeBr2);ironbromide(febr2);IRON (II) BROMIDE;IRON BROMIDE;FERROUS BROMIDE;iron dibromide;Ironbromideanhydrousorangepowder
• CAS NO: 7789-46-0
• Molecular Formula: Br2Fe
• Molecular Weight: 215.65
• EINECS: 232-168-8
• Product Categories: metal halide;26: Fe;Beaded Materials;Crystal Grade Inorganics;Fe;Iron;Iron Salts;Materials Science;Metal and Ceramic Science;Salts;Ultra-High Purity Materials
• Mol File: 7789-46-0.mol
• Article Data: 18

Chemical Properties

• Melting Point: 684 °C(lit.)
• Boiling Point: 934 °C(lit.)
• Appearance: Yellow/beads
• Density: 4.63 g/mL at 25 °C(lit.)
• Solubility: ethanol: very soluble(lit.)
• Water Solubility: Soluble in water, THF, methanol, ethanol.
• Sensitive: Hygroscopic
• Stability: hygroscopic
• Merck: 14,4042
• CAS DataBase Reference: IRON (II) BROMIDE(CAS DataBase Reference)
• NIST Chemistry Reference: IRON (II) BROMIDE(7789-46-0)
• EPA Substance Registry System: IRON (II) BROMIDE(7789-46-0)

Safety Data

• Hazard Codes: Xn
• Statements: 20-36/37/38
• Safety Statements: 26-36
• RIDADR: UN3260
• WGK Germany: 3
• TSCA: Yes
• HazardClass: 8
• PackingGroup: III
• Hazardous Substances Data: 7789-46-0(Hazardous Substances Data)

Usage

Chemical Properties

Different sources of media describe the Chemical Properties of 7789-46-0 differently. You can refer to the following data:
1. Yellow to dark brown lumps
2. In contrast to the chloride, iron(III) bromide is unstable under these conditions. The hydrated bromide can be dehydrated in a stream of hydrogen bromide at 400°C. Iron(II) bromide forms a layer lattice of the CdI2 type. It has a magnetic moment,μeff= 5·71 B.M. at 295°K. It is deliquescent and very soluble in water; the pale green hexahydrate crystallizes at room temperature, the tetrahydrate above 49°C and the dihydrate above 83°C. A 9-hydrate forms below -29·3°C. The anhydrous salt is also soluble in ether, ethanol and acetonitrile.

Uses

Iron(II) bromide is used as a polymerization catalyst. It is used in water treatment, chemical analysis and in ultra high purity for certain crystal growth applications.

Preparation

Iron(II) bromide can be prepared by the direct reaction of bromine or hydrogen bromide with iron at red heat.

General Description

This product has been enhanced for catalytic efficiency.

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

Upstream product

• 10035-10-6 hydrogen bromide 
• 7439-89-6 iron 
• 7726-95-6 bromine 
• 13463-40-6 iron pentacarbonyl 
• 7558-02-3 potassium bromide 
• 10097-32-2 bromine 
• 10031-26-2 iron (III) bromide 
• 10031-26-2 ferric(III) bromide 
• 10102-43-9 nitrogen(II) oxide 
• 18475-84-8 iron(II) carbonyl dibromide 

Downstream Products

• 70318-01-3 Fe(P(OCH₃)3)5Br⁽¹⁺⁾*B(C₆H₅)4^(1-)=[Fe(P(OCH₃)3)5Br][B(C₆H₅)4] 
• 70323-65-8 Fe(P(OC₂H₅)3)5Br⁽¹⁺⁾*B(C₆H₅)4^(1-)=[Fe(P(OC₂H₅)3)5Br][B(C₆H₅)4] 
• 94841-57-3 2-(((3-(1-imidazolyl)propyl)carbamoyloxy)methyl)-5,10,15,20-tetrakis(α,α,α,α-o-pivalamidophenyl)porphyrinatoiron(III) bromide 
• 73450-20-1 [Fe(tris(3,5-dimethyl-1-pyrazolylmethyl)amine)Br]BPh₄ 

Relevant articles and documents

Observation of Single-Ion. Transitions in the Ordered States of FeBr2

By utilizing a far infrared laser operating in the THz range, we have observed new electron spin resonance (ESR) lines in the ordered states of a layered antiferromagnet with strong uniaxial anisotropy, FeBr2. We interpret these ESR lines as arising from transitions within the lowest triplet state of single Fe2+ ions. Good agreement between theory and experiment is obtained without any adjustable parameters.

Neutron-scattering studies of a phase transition in the metamagnet FeBr2 under external magnetic fields

Neutron-scattering experiments have been performed on the metamagnet FeBr2 under external magnetic fields. We find an anomaly in the temperature (T) and magnetic-field (H) dependences of the intensity of the (2,0,1/2) antiferromagnetic Bragg scattering at the temperature T1(H) at which an anomaly in specific heat has been observed in addition to the anomaly at the Neel temperature TN(H). We argue that our results are consistent with the theoretical H-T phase diagram of a metamagnet in which the tricritical point decomposes into a critical end point and a bicritical end point. We locate the latter point at Tcr? 10.8 K and Hcr? 1.4 T in this compound.

How Inert, Perturbing, or Interacting Are Cryogenic Matrices? A Combined Spectroscopic (Infrared, Electronic, and X-ray Absorption) and DFT Investigation of Matrix-Isolated Iron, Cobalt, Nickel, and Zinc Dibromides

The interactions of FeBr2, CoBr2, NiBr2, and ZnBr2 with Ne, Ar, Kr, Xe, CH4, and N2 matrices have been investigated using IR, electronic absorption, and X-ray absorption spectroscopies as well as DFT calculations. ZnBr2 is linear in all of the matrices. NiBr2 is linear in all but N2 matrices, where it is severely bent. For FeBr2 and CoBr2 there is a more gradual change, with evidence of nonlinearity in Xe and CH4 matrices as well as N2. In the N2 matrices, the presence of νNN modes blue-shifted from the "free" N2 values indicates the presence of physisorbed species, and the magnitude of the blue shift correlates with the shift in the ν3 mode of the metal dibromide. In the case of NiCl2 and NiBr2, chemisorbed species are formed after photolysis, but only if deposition takes place below 10 K. There was no evidence for chemisorbed species for NiF2 and FeBr2, and in the case of CoBr2 the evidence was not strong.

Microwave-assisted carbohydrohalogenation of first-row transition-metal oxides (M = V, Cr, Mn, Fe, Co, Ni, Cu) with the formation of element halides

The anhydrous forms of first-row transition-metal chlorides and bromides ranging from vanadium to copper were synthesized in a one-step reaction using the relatively inexpensive element oxides, carbon sources, and halogen halides as starting materials. The reactions were carried out in a microwave oven to give quantitative yields within short reaction times.