Bromine trifluoride
Chemical compound From Wikipedia, the free encyclopedia
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Chemical compound From Wikipedia, the free encyclopedia
Bromine trifluoride is an interhalogen compound with the formula BrF3. At room temperature, it is a straw-coloured liquid with a pungent odor[5] 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.[6]
Identifiers | |
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3D model (JSmol) |
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ChemSpider | |
ECHA InfoCard | 100.029.211 |
EC Number |
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PubChem CID |
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UNII | |
UN number | 1746 |
CompTox Dashboard (EPA) |
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Properties | |
BrF3 | |
Molar mass | 136.90 g/mol |
Appearance | straw-coloured liquid hygroscopic |
Odor | Choking, pungent[1] |
Density | 2.803 g/cm3 [2] |
Melting point | 8.77 °C (47.79 °F; 281.92 K) |
Boiling point | 125.72 °C (258.30 °F; 398.87 K) |
Reacts with water[3] | |
Structure | |
T-shaped (C2v) | |
1.19 D | |
Hazards[4] | |
Occupational safety and health (OHS/OSH): | |
Main hazards |
Reacts violently with water to release HF, highly toxic, corrosive, powerful oxidizer |
GHS labelling: | |
Danger | |
H271, H300+H310+H330, H314, H373 | |
P102, P103, P210, P220, P221, P260, P264, P271, P280, P283, P284, P301+P310, P301+P330+P331, P303+P361+P353, P304+P312, P305+P351+P338+P310, P306+P360, P308+P313, P340, P363, P370+P380 | |
NFPA 704 (fire diamond) | |
Safety data sheet (SDS) | http://www.chammascutters.com/en/downloads/Bromine-Trifluoride-MSDS.pdf |
Related compounds | |
Other anions |
Bromine monochloride |
Other cations |
Chlorine trifluoride Iodine trifluoride |
Related compounds |
Bromine monofluoride Bromine pentafluoride |
Supplementary data page | |
Bromine trifluoride (data page) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Bromine trifluoride was first described by Paul Lebeau in 1906, who obtained the material by the reaction of bromine with fluorine at 20 °C:[7]
The disproportionation of bromine monofluoride also gives bromine trifluoride:[5]
Like ClF3 and IF3, the BrF3 molecule is T-shaped and planar. In the VSEPR formalism, the bromine center is assigned two electron lone pairs. The distance from the bromine atom to each axial fluorine atom is 1.81 Å and to the equatorial fluorine atom is 1.72 Å. The angle between an axial fluorine atom and the equatorial fluorine atom 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.[8][9]
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.[10] Already at -196 °C, it reacts with acetonitrile to give 1,1,1-trifluoroethane.[11]
The liquid is conducting, owing to autoionisation:[6]
Fluoride salts dissolve readily in BrF3 forming tetrafluorobromate:[6]
It reacts as a fluoride donor:[12]
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