Английская Википедия:Bromine trifluoride
Bromine trifluoride is an interhalogen compound with the formula BrF3. At room temperature, it is a straw-coloured liquid with a pungent odor[1] which decomposes violently on contact with water and organic compounds. It is a powerful fluorinating agent and an ionizing inorganic solvent. It is used to produce uranium hexafluoride (UF6) in the processing and reprocessing of nuclear fuel.[2]
Synthesis
Bromine trifluoride was first described by Paul Lebeau in 1906, who obtained the material by the reaction of bromine with fluorine at 20 °C:[3]
The disproportionation of bromine monofluoride also gives bromine trifluoride:[1]
Structure
Like ClF3 and IF3, the BrF3 molecule is T-shaped and planar. In the VSEPR formalism, the bromine center is assigned two electron pairs. 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.[4][5]
Chemical properties
In a highly exothermic reaction, BrF3 reacts with water to form hydrobromic acid and hydrofluoric acid:
BrF3 is a fluorinating agent, but less reactive than ClF3.[6] Already at -196 °C, it reacts with acetonitrile to give 1,1,1-trifluoroethane.[7]
- Шаблон:Chem2 + Шаблон:Frac Br2 + Шаблон:Frac N2
The liquid is conducting, owing to autoionisation:[2]
Fluoride salts dissolve readily in BrF3 forming tetrafluorobromate:[2]
It reacts as a fluoride donor:[8]
References
External links
Шаблон:Bromine compounds Шаблон:Fluorine compounds
- ↑ 1,0 1,1 Шаблон:Cite book
- ↑ 2,0 2,1 2,2 Шаблон:Greenwood&Earnshaw
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite book
- ↑ Шаблон:Cite journal
- ↑ A. J. Edwards and G. R. Jones. J. Chem. Soc. A, 1467 (1969)