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Bromine pentafluoride Structure and dimensions of the bromine pentafluoride molecule in the gas phase Ball-and-stick model of bromine pentafluoride Space-filling model of bromine pentafluoride Names IUPAC nameBromine pentafluoride
Identifiers CAS Number3D model (
JSmol)
ChemSpiderInChI=1S/BrF5/c2-1(3,4,5)6
YKey: XHVUVQAANZKEKF-UHFFFAOYSA-N
YInChI=1/BrF5/c2-1(3,4,5)6
Key: XHVUVQAANZKEKF-UHFFFAOYAC
FBr(F)(F)(F)F
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) 4 0 3 W(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 Related compoundsOther
anions Bromine monochlorideOther
cations Chlorine pentafluorideRelated
compounds Bromine monofluorideExcept 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 referencesChemical 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.
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:
For the preparation of smaller amounts, potassium bromide is used:[3]
This route yields BrF5 almost completely free of trifluorides and other impurities.[3]
BrF5 reacts with water to form bromic acid and hydrofluoric acid:[4]
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:
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]
Salts and covalent derivatives of the
fluorideion
HF ?HeF2 LiF BeF2 BFRetroSearch is an open source project built by @garambo | Open a GitHub Issue
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