Chemistry:Bromine trifluoride

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Bromine trifluoride
Structural formula, showing bond lengths and angles
Bromine Trifluoride
Identifiers
3D model (JSmol)
ChemSpider
EC Number
  • 232-132-1
UNII
UN number 1746
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]
Main hazards Reacts violently with water to release HF, highly toxic, corrosive, powerful oxidizer
Safety data sheet http://www.chammascutters.com/en/downloads/Bromine-Trifluoride-MSDS.pdf
GHS pictograms GHS03: OxidizingGHS05: CorrosiveGHS06: ToxicGHS08: Health hazard
GHS Signal word Danger
H271, H300+310+330Script error: No such module "Preview warning".Category:GHS errors, H314, H373
P102, P103, P210, P220, P221, P260, P264, P271, P280, P283, P284, P301+310, P301+330+331, P303+361+353, P304+312, P306+360, P308+313, P370+380, P340, P363, P305+351+338+310
NFPA 704 (fire diamond)
Related compounds
Other anions
Bromine monochloride
Other cations
Chlorine trifluoride
Iodine trifluoride
Related compounds
Bromine monofluoride
Bromine pentafluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
Tracking categories (test):

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]

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:[7]

Br
2
+ 3 F
2
→ 2 BrF
3

The disproportionation of bromine monofluoride also gives bromine trifluoride:[5]

3 BrF → BrF
3
+ Br
2

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.[8][9]

Chemical properties

In a highly exothermic reaction, BrF3 reacts with water to form hydrobromic acid and hydrofluoric acid:

BrF
3
+ 2 H
2
O → 3 HF + HBr + O
2

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]

BrF
3
+ CH
3
CN → CH
3
CF
3
+ ​12 Br2 + ​12 N2

The liquid is conducting, owing to autoionisation:[6]

2 BrF
3
⇌ BrF+
2
+ BrF
4

Fluoride salts dissolve readily in BrF3 forming tetrafluorobromate:[6]

KF + BrF
3
→ KBrF
4

It reacts as a fluoride donor:[12]

BrF
3
+ SbF
5
→ [BrF+
2
][SbF
6
]

References

  1. "Safety Data Sheet : Bromine Trifluoride" (PDF). http://www.chammascutters.com/en/downloads/Bromine-Trifluoride-MSDS.pdf. 
  2. Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3. 
  3. "Archived copy". http://www.mathesongas.com/pdfs/msds/MAT03380.pdf. 
  4. "Safety Data Sheet Bromine Trifluoride". Airgas. https://www.airgas.com/msds/001112.pdf. 
  5. 5.0 5.1 Simons JH (1950). "Bromine(III) Fluoride (Bromine Trifluoride)". Bromine (III) Fluoride - Bromine Trifluoride. Inorganic Syntheses. 3. pp. 184–186. doi:10.1002/9780470132340.ch48. ISBN 978-0-470-13234-0. 
  6. 6.0 6.1 6.2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. 
  7. Lebeau P. (1906). "The effect of fluorine on chloride and on bromine". Annales de Chimie et de Physique 9: 241–263. 
  8. Gutmann V (1950). "Die Chemie in Bromitrifluorid". Angewandte Chemie 62 (13–14): 312–315. doi:10.1002/ange.19500621305. Bibcode1950AngCh..62..312G. 
  9. Meinert H (1967). "Interhalogenverbindungen". Zeitschrift für Chemie 7 (2): 41–57. doi:10.1002/zfch.19670070202. 
  10. Rozen, Shlomo; Sasson, Revital (2007). "Bromine Trifluoride". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/9780470842898.rb266.pub2. ISBN 978-0471936237. 
  11. Rozen, Shlomo (2010). "Selective Reactions of Bromine Trifluoride in Organic Chemistry". Advanced Synthesis & Catalysis 352 (16): 2691–2707. doi:10.1002/adsc.201000482. 
  12. A. J. Edwards and G. R. Jones. J. Chem. Soc. A, 1467 (1969)

External links