Bromine trifluoride
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2008-05-27T17:39:02Z
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{{Chembox new
| ImageFile = Bromine-trifluoride-3D-vdW.png
| ImageSize = 150px
| ImageName = Bromine trifluoride
| Section2 = {{Chembox Properties
| Formula = BrF<sub>3</sub>
| 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 [[Debye|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]]<br />[[Iodine trifluoride]]
| OtherCpds = [[Bromine monofluoride]]<br />[[Bromine pentafluoride]]
}}
}}
'''Bromine trifluoride''' is a highly [[toxic]] and corrosive [[fluoride]] of [[bromine]] with [[chemical formula]] BrF<sub>3</sub>. It was discovered by [[Paul Lebeau]] in 1906.<ref name="lebeau">{{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}}</ref> It occurs as a colorless, [[yellow]], or [[gray]] fuming [[liquid]] with an irritating [[odor]]. It is soluble in [[sulfuric acid]] but may [[explode]] on contact with [[water]]. While it is a potent fluorinating agent it is less reactive than [[chlorine trifluoride|ClF<sub>3</sub>]]. It is used to produce [[uranium hexafluoride]], UF<sub>6</sub> in the processing and reprocessing of nuclear fuel.<ref name = "Greenwood">{{Greenwood&Earnshaw}}</ref>
==Synthesis==
Bromine trifluoride can be obtained by the reaction of [[bromine]] with [[fluorine]] at 20 °C.
:Br<sub>2</sub> + 3F<sub>2</sub> → 2BrF<sub>3</sub>
The [[disproportionation]] of [[bromine monofluoride]] is also a source for bromine trifluoride.
:3BrF → BrF<sub>3</sub> + Br<sub>2</sub><ref name="simons">{{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}}</ref>
==Structure==
[[Image:Bromine-trifluoride-chemical-structure.png|120px|Bromine-trifluoride-chemical-structure]]
Like ClF<sub>3</sub> and IF<sub>3</sub> the BrF<sub>3</sub> [[molecule]] is T-shaped. With the two [[Lone pair|electron pairs]] the [[coordination number]] is 5. The distance from the bromine each axial fluorine is 1.81 [[Ångström|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 [[Lone pair|electron pair]]s being greater than that of the Br-F bonds.<ref name="gutmann">{{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}}</ref><ref name="meinert">{{cite journal | author= Meinert H| title= Interhalogenverbindungen | journal=Zeitschrift für Chemie| year=1967 | volume=7 | pages=41}}</ref>
==Chemistry and Properties==
Liquid BrF3 is conducting and this is attributed to dissociation:<ref name = "Greenwood"/>
:BrF3 {{unicode|⇌}} BrF<sub>2</sub><sup>+</sup> + BrF<sub>4</sub><sup><nowiki>−</nowiki></sup>
Many ionic fluorides dissolve readily in BrF<sub>3</sub> forming solvobases<ref name = "Greenwood"/> e.g.
:KF + BrF<sub>3</sub> → KBrF<sub>4</sub>
==References==
<div class="references-small"><references /></div>
[[Category:Bromine compounds]]
[[Category:Fluorides]]
[[Category:Interhalogen compounds]]
[[de:Brom(III)-fluorid]]
[[pt:Trifluoreto de bromo]]
[[ru:Трифторид брома]]