Bromine trifluoride 2317010 215315340 2008-05-27T17:39:02Z DOI bot 6652755 Citation maintenance. You can [[WP:DOI|use this bot]] yourself! Please [[User:DOI_bot/bugs|report any bugs]]. {{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&nbsp;g/ml,&nbsp;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|&#8652;}} BrF<sub>2</sub><sup>+</sup> + BrF<sub>4</sub><sup><nowiki>&minus;</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]]