Bromine trifluoride
Structural formula, showing bond lengths and angles | |
Bromine Trifluoride | |
Identifiers | |
---|---|
7787-71-5 | |
PubChem | 24594 |
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) |
decomposes violently[3] | |
Solubility in sulfuric acid | very soluble |
Structure | |
T-shaped (C2v) | |
1.19 D | |
Vapor pressure | {{{value}}} |
Related compounds | |
Other anions
|
Bromine monochloride |
Other cations
|
Chlorine trifluoride Iodine trifluoride |
Related compounds
|
Bromine monofluoride Bromine pentafluoride |
Supplementary data page | |
Refractive index (n), Dielectric constant (εr), etc. |
|
Thermodynamic
data |
Phase behaviour solid–liquid–gas |
UV, IR, NMR, MS | |
verify (what is ?) | |
Infobox references | |
Bromine trifluoride is an interhalogen compound with the formula BrF3. It is a straw-coloured liquid with a pungent odor.[4] It is soluble in sulfuric acid but explodes 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.[5]
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:[6]
- Br2 + 3 F2 → 2 BrF3
The disproportionation of bromine monofluoride also gives bromine trifluoride:[4]
- 3 BrF → BrF3 + Br2
Structure
Like ClF3 and IF3, the BrF3 molecule is T-shaped. 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.[7][8]
Chemical properties
BrF3 is a fluorinating agent, but less reactive than ClF3. The liquid is conducting, owing to autoionisation:[5]
- 2 BrF3 ⇌ BrF2+ + BrF4−
Many ionic fluorides dissolve readily in BrF3 forming fluoroanions:[5]
- KF + BrF3 → KBrF4
References
- ↑ http://www.chammascutters.com/en/downloads/Bromine-Trifluoride-MSDS.pdf
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- ↑ http://www.mathesongas.com/pdfs/msds/MAT03380.pdf
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External links
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- Bromine compounds
- Fluorides
- Interhalogen compounds
- Fluorinating agents
- Oxidizing agents