Bromine pentafluoride

Space-filling model of bromine pentafluoride

Names

IUPAC name

Bromine pentafluoride

Identifiers

CAS Number

7789-30-2^Y

3D model (JSmol)

Interactive image

ChemSpider

23008^Y

ECHA InfoCard

100.029.234

EC Number

232-157-8

PubChem CID

24606

RTECS number

EF9350000

UNII

UPI6B7Y9UQ

UN number

1745

CompTox Dashboard (EPA)

DTXSID30894171

InChI

InChI=1S/BrF5/c2-1(3,4,5)6^Y
Key: XHVUVQAANZKEKF-UHFFFAOYSA-N^Y
InChI=1/BrF5/c2-1(3,4,5)6
Key: XHVUVQAANZKEKF-UHFFFAOYAC

SMILES

FBr(F)(F)(F)F

Properties

Chemical formula

BrF₅

Molar mass

174.894 g.mol⁻¹

Appearance

Pale yellow liquid

Density

2.466 g/cm³

Melting point

−61.30 °C (−78.34 °F; 211.85 K)

Boiling point

40.25 °C (104.45 °F; 313.40 K)

Solubility in water

Reacts with water

Structure

Molecular shape

Square pyramidal

Hazards

Occupational safety and health (OHS/OSH):

Main hazards

Powerful oxidizer, corrosive, highly toxic, reacts violently with water to release HF^[1]

GHS labelling:

Pictograms

Signal word

Danger

Hazard statements

H271, H300+H310+H330, H314, H372

Precautionary statements

P210, P220, P221, P260, P264, P270, P271, P280, P283, P284, P301+P310, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P306+P360, P307+P311, P309+P311, P310, P314, P320, P321, P331, P363, P370+P378, P371+P380+P375, P403+P233, P405, P501

NFPA 704 (fire diamond)

W
OX

Flash point

Non-flammable

NIOSH (US health exposure limits):

PEL (Permissible)

none^[1]

REL (Recommended)

TWA 0.1 ppm (0.7 mg/m³)^[1]

IDLH (Immediate danger)

N.D.^[1]

Safety data sheet (SDS)

External MSDS^{[dead link]}

Related compounds

Other anions

Bromine monochloride

Other cations

Chlorine pentafluoride
Iodine pentafluoride

Related compounds

Bromine monofluoride
Bromine trifluoride

Supplementary data page

Bromine pentafluoride (data page)

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Y verify (what is ^YN ?)

Infobox references

Chemical compound

Bromine pentafluoride, BrF₅, is an interhalogen compound and a fluoride of bromine. It is a strong fluorinating agent.

BrF₅ finds use in oxygen isotope analysis. Laser ablation of solid silicates in the presence of BrF₅ releases O₂ for subsequent analysis.^[2] It has also been tested as an oxidizer in liquid rocket propellants and is used as a fluorinating agent in the processing of uranium.

Preparation

BrF₅ was first prepared in 1931 by the direct reaction of bromine and fluorine.^[3] This reaction is suitable for the preparation of large quantities,^{[citation needed]} and is carried out at temperatures over 150 °C (302 °F) with an excess of fluorine:

Br₂ + 5 F₂ → 2 BrF₅

For the preparation of smaller amounts, potassium bromide is used:^[3]

KBr + 3 F₂ → KF + BrF₅

This route yields BrF₅ almost completely free of trifluorides and other impurities.^[3]

Reactions

BrF₅ reacts with water to form bromic acid and hydrofluoric acid:^[4]

BrF₅ + 3 H₂O → HBrO₃ + 5 HF

It is an extremely effective fluorinating agent, being able to convert most metals to their highest fluorides even at room temperature. With uranium and uranium compounds, it can be used to produce uranium hexafluoride:

5 U + 6 BrF₅ → 5 UF₆ + 3 Br₂

Hazards

BrF₅ reacts violently with water, and is severely corrosive and toxic. Its vapors are also extremely irritating to all parts of the human body, especially the skin, eyes and other mucous membranes. Like many other interhalogen compounds, it will release "smoke" containing acidic vapors if exposed to moist air, which comes from its reaction with the water in the air. Exposure to 100 ppm or more for more than one minute is lethal to most experimental animals. Chronic exposure may cause kidney damage and liver failure.^[5]

Additionally, BrF₅ is a strong oxidizing agent and may spontaneously ignite or explode upon contact with flammable substances such as organic materials and metal dust.^[5]

References

^ ^a ^b ^c ^d NIOSH Pocket Guide to Chemical Hazards. "#0065". National Institute for Occupational Safety and Health (NIOSH).
^ Clayton, R.; Mayeda, T. K. (1963). "The use of bromine pentafluoride in the extraction of oxygen from oxides and silicates for isotopic analysis". Geochimica et Cosmochimica Acta. 27 (1): 43–48. Bibcode:1963GeCoA..27...43C. doi:10.1016/0016-7037(63)90071-1.
^ ^a ^b ^c Hyde, G. A.; Boudakian, M. M. (1968). "Synthesis routes to chlorine and bromine pentafluorides". Inorganic Chemistry. 7 (12): 2648–2649. doi:10.1021/ic50070a039.
^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 834. ISBN 978-0-08-037941-8.
^ ^a ^b Patnaik, Pradyot (2007). A comprehensive guide to the hazardous properties of chemical substances (3rd ed.). Wiley-Interscience. p. 480. ISBN 978-0-471-71458-3.

External links

WebBook page for BrF₅
International Chemical Safety Card 0974
NIOSH Pocket Guide to Chemical Hazards. "#0065". National Institute for Occupational Safety and Health (NIOSH).
National Pollutant Inventory - Fluoride and compounds fact sheet

Bromine compounds

Br(−I)