Bromine trifluoride

Structural formula
General
Surname	Bromine trifluoride
other names	Bromine (III) fluoride
Molecular formula	BrF 3
Brief description	colorless to yellowish liquid
External identifiers / databases
CAS number 7787-71-5 EC number 232-132-1 ECHA InfoCard 100.029.211 PubChem 24594 Wikidata Q419784
properties
Molar mass	136.90 g mol −1
Physical state	liquid
density	2.84 g ml −1
Melting point	8.77 ° C
boiling point	125.72 ° C
solubility	Violent reaction with water
Refractive index	1.4536 (25 ° C)
safety instructions
GHS hazard labeling no classification available
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . Refractive index: Na-D line , 20 ° C

Bromine trifluoride is a colorless to yellowish liquid which chemically represents a connection between the halogens bromine and fluorine . It was discovered in 1906 by Paul Lebeau . It is an interhalogen compound .

Extraction and presentation

Bromine trifluoride can be obtained by reacting bromine with fluorine.

${\displaystyle \mathrm {Br_{2}+3\ F_{2}\longrightarrow 2\ BrF_{3}} }$

The representation by disproportionation of bromine fluoride is also possible.

${\displaystyle \mathrm {3\ BrF\longrightarrow BrF_{3}+Br_{2}} }$

Very pure bromine trifluoride can be obtained by direct fluorination of bromine with trichlorofluoromethane at −40 ° C.

properties

Bromine trifluoride is a colorless liquid that smokes in air. It is very reactive and attacks the skin heavily. Even quartz and other silicates are noticeably attacked at 30 ° C. In solid form, it is in the form of long prisms. The critical temperature is 327 ° C.

Similar to chlorine trifluoride and iodine trifluoride , bromine trifluoride is a T-shaped molecule. The distance between bromine and the axial fluorine is 181 pm in each case  , while the distance to the central fluorine is 172 pm. The angle between the central and axial fluorine is 86.2 °.

use

Bromine trifluoride is a good solvent for reactions that take place under highly oxidizing conditions. It is also a strong fluorinating agent and can be used for the synthesis of corresponding organic and inorganic compounds.

Individual evidence

1. ↑ ^{a b c} Entry on Bromofluoride. In: Römpp Online . Georg Thieme Verlag, accessed on May 26, 2014.
2. ^ ^{A b} A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 .
3. ↑ ^{a b c} J. H. Simons: Bromine (III) fluoride . In: Ludwig F. Audrieth (Ed.): Inorganic Syntheses . tape 3 . McGraw-Hill, Inc., 1950, pp. 184-186 (English).
4. ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Index of Refraction of Inorganic Liquids, pp. 4-140.
5. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
6. ↑ ^{a b c} Georg Brauer (ed.), With the collaboration of Marianne Baudler a . a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 169.
7. ↑ Kirk-Othmer Encyclopedia of Chemical Technology: Bromine, Inorganic Compounds ( Memento of the original from September 30, 2007 in the Internet Archive ) Info: The archive link was automatically inserted and not yet checked. Please check the original and archive link according to the instructions and then remove this notice. .