Bromine pentafluoride
Structure and dimensions of the bromine pentafluoride molecule in the gas phase | |||
|
|||
Names | |||
---|---|---|---|
IUPAC name
Bromine pentafluoride
|
|||
Identifiers | |||
7789-30-2 | |||
ChemSpider | 23008 | ||
Jmol 3D model | Interactive image | ||
PubChem | 24606 | ||
RTECS number | EF9350000 | ||
|
|||
|
|||
Properties | |||
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) | ||
reacts | |||
Structure | |||
Square pyramidal | |||
Vapor pressure | {{{value}}} | ||
Related compounds | |||
Other anions
|
Bromine monochloride | ||
Other cations
|
Chlorine pentafluoride Iodine pentafluoride |
||
Related compounds
|
Bromine monofluoride Bromine trifluoride |
||
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 pentafluoride, BrF5, is an interhalogen compound and a fluoride of bromine. It is a strong fluorination reagent.
BrF5 finds use in oxygen isotope analysis. Laser ablation of solid silicates in the presence of bromine pentafluoride releases O2 for subsequent analysis.[1] 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
Bromine pentafluoride was first prepared in 1931 by the direct reaction of bromine with fluorine.[2] This reaction is suitable for the preparation of large quantities, 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:[2]
- KBr + 3 F2 → KF + BrF5
This route yields bromine pentafluoride almost completely free of trifluorides and other impurities.[2]
Reactions
Bromine pentafluoride reacts explosively with water, but when moderated by dilution with acetonitrile, it will form bromic acid and hydrofluoric acid, simple hydrolysis products:[3]
- BrF5 + 3 H2O → HBrO3 + 5 HF
It is an extremely effective fluorinating agent, converting most uranium compounds to the hexafluoride at room temperature.
Hazards
Bromine pentafluoride is severely corrosive to the skin, and its vapors are irritating to the eyes, skin, and mucous membranes. Exposure to 100 ppm for a few minutes is lethal to most experimental animals. Chronic exposure may cause nephrosis and hepatosis.[4]
It may spontaneously ignite or explode upon contact with organic materials or metals in powdered form.[4]
References
External links
- WebBook page for BrF5
- International Chemical Safety Card 0974
- Lua error in package.lua at line 80: module 'strict' not found.
- National Pollutant Inventory - Fluoride and compounds fact sheet
- Pages with broken file links
- Articles without EBI source
- Articles without KEGG source
- Articles without UNII source
- Pages using collapsible list with both background and text-align in titlestyle
- Chemical articles using a fixed chemical formula
- Chemical articles having a data page
- Fluorides
- Bromine compounds
- Interhalogen compounds
- Fluorinating agents
- Oxidizing agents