Bromine trifluoride

Chembox new
ImageFile = Bromine-trifluoride-3D-vdW.png ImageSize = 150px
ImageName = Bromine trifluoride
Section2 = Chembox Properties
Formula = BrF₃
MolarMass = 136.90 g/mol
Appearance = straw-coloured liquid
Density = 2.8 g/ml, liquid
Solubility = "decomposes"
MeltingPt = 8.8 °C
BoilingPt = 125.8 °C
Viscosity =
Section3 = Chembox Structure
MolShape = T-shaped
Dipole = 1.19 D
Section7 = Chembox Hazards
ExternalMSDS =
EUClass = not listed
NFPA-H = 3
NFPA-F =
NFPA-R = 3 | NFPA-O = OX
Section8 = Chembox Related
OtherAnions = Bromine monochloride
OtherCations = Chlorine trifluoride
Iodine trifluoride
OtherCpds = Bromine monofluoride
Bromine pentafluoride

Bromine trifluoride is the inorganic compound with the formula BrF₃. This toxic, colourless, and corrosive liquid is soluble in sulfuric acid but explodes on contact with water and organic compounds. It is a potent fluorinating agent and an ionizing inorganic solvent. It is used to produce uranium hexafluoride, UF₆ in the processing and reprocessing of nuclear fuel.Greenwood&Earnshaw]

ynthesis

Bromine trifluoride was first described by Paul Lebeau in 1906, who obtained the material by the reaction of bromine with fluorine at 20 °C:cite journal | author= Lebeau P. | title= The effect of fluorine on chloride and on bromine | journal=Annales de Chimie et de Physique| year=1906 | volume=9 | pages=241–263] :Br₂ + 3 F₂ → 2 BrF₃

The disproportionation of bromine monofluoride also gives bromine trifluoride:cite journal | author= Simons JH| title= Bromine (III) Fluoride - Bromine Trifluoride | journal=Inorganic Synthesis| year=1950 | volume=3 | pages=184–186| doi= 10.1002/9780470132340.ch48] :3 BrF → BrF₃ + Br₂

tructure

Like ClF₃ and IF₃ the BrF₃ molecule is T-shaped. In the VSEPR formalism, the bromine center is assigned two electron pairs leading to a coordination number of 5. The distance from the bromine each axial fluorine is 1.81 Å and to the equatorial fluorine is 1.72 Å. The angle between an axial fluorine and the equatorial fluorine is slightly smaller than 90° — the 86.2° angle observed is due to the repulsion generated by the electron pairs being greater than that of the Br-F bonds.cite journal | author= Gutmann V| title= Die Chemie in Bromtrifuoride | journal=Angewante Chemie| year=1950 | volume=62 | pages=312–315| doi= 10.1002/ange.19500621305] cite journal | author= Meinert H| title= Interhalogenverbindungen | journal=Zeitschrift für Chemie| year=1967 | volume=7 | pages=41]

Chemical properties

BrF3 is a fluorinating agent, but less reactive than ClF₃. The liquid is conducting, owing to "autoionization"::2 BrF3 unicode| BrF₂⁺ + BrF₄⁻Many ionic fluorides dissolve readily in BrF₃ forming solvobases e.g. :KF + BrF₃ → KBrF₄

References

External links

* [http://webbook.nist.gov/cgi/cbook.cgi?ID=C7787715 WebBook page for BrF3]