- 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 insulfuric acid but explodes on contact withwater and organic compounds. It is a potent fluorinating agent and an ionizing inorganic solvent. It is used to produceuranium 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 ofbromine withfluorine 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 BrF3The
disproportionation ofbromine 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 + Br2tructure
Like ClF3 and IF3 the BrF3
molecule is T-shaped. In theVSEPR formalism, the bromine center is assigned two electron pairs leading to acoordination 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 → KBrF4References
External links
* [http://webbook.nist.gov/cgi/cbook.cgi?ID=C7787715 WebBook page for BrF3]
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