Bromine chloride

Structural formula
General
Surname	Bromine chloride
other names	Bromine monochloride
Molecular formula	BrCl
Brief description	red-brown gas
External identifiers / databases
CAS number 13863-41-7 EC number 237-601-4 ECHA InfoCard 100.034.169 PubChem 61697 Wikidata Q421222
properties
Molar mass	115.35 g mol −1
Physical state	gaseous
density	3.129 g cm −3 (−140 ° C)
Melting point	−54 ° C
boiling point	−5 ° C (decomposition 10 ° C)
Vapor pressure	20 Torr (−50 ° C)
solubility	hydrolysis occurs in water
Dipole moment	0.519 (4) D (1.7 x 10 -30  C  ·  m )
safety instructions
GHS labeling of hazardous substances danger H and P phrases H: 314-331 P: ?
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Bromine chloride is a gaseous interhalogen compound that consists of the elements bromine and chlorine . In this compound, bromine formally has the +1 oxidation state. It is a covalent bond.

history

First investigations of the melting and boiling curves of mixtures of chlorine and bromine were published as early as the beginning of the 20th century, whereby no compound formation was detectable. Later, some authors described observations that indicated the possible existence of a bromine-chlorine compound, whereby neither the composition could be clarified nor a production could be realized. The first proof of bromine chloride by comparing vapor pressure curves and isolating the pure compound was achieved by Hermann Lux in 1930.

Manufacturing

The first production of bromine chloride was carried out by Hermann Lux by slow distillation of a chlorine-bromine mixture at −70 ° C. The connection can be established by UV irradiation of a chlorine-bromine mixture in halogenated hydrocarbons (CF _n Cl _{4− n} ).

properties

In the solid state, bromine chloride is an ocher-yellow substance that melts sharply at −54 ° C. In comparison, a 1: 1 mixture of chlorine and bromine melts in the range between -66 ° C and -52 ° C. Deviating melting point data for bromine chloride by other authors at −66 ° C or −75 ° C may be based on measurements on mixtures of the elements. The ocher-yellow melt boils under normal pressure at −5 ° C, with decomposition of the compound being observed from 10 ° C. Zigzag-shaped BrCl chains are formed in the crystal lattice. The compound crystallizes in an orthorhombic crystal lattice with the space group Cmc 2 ₁ (space group no. 36) .

In water, the compound hydrolyzes to form hypobromous acid and hydrochloric acid .

${\displaystyle \mathrm {BrCl+H_{2}O\rightarrow HOBr+HCl} }$

In the presence of an excess of chloride ions, compounds with the polyhalide ion BrCl ₂ ^- can be obtained.

${\displaystyle \mathrm {BrCl+Cl^{-}\rightleftharpoons {BrCl_{2}}^{-}} }$

use

Bromine chloride is used in the manufacture of lithium-sulfur dioxide batteries . It is also used as an active ingredient in disinfectants , fungicides and algicides .

Individual evidence

1. ^ ^{A b c} A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 466.
2. ↑ ^{a b c} T. Drews, K. Seppelt: Bromine Monofluoride. In: Z. Anorg. General Chem. 638, 2012, pp. 2106-2110, doi: 10.1002 / zaac.201200293 .
3. ↑ ^{a b c d e} Entry on bromine chloride in the GESTIS substance database of the IFA , accessed on February 1, 2016(JavaScript required) .
4. ↑ ^{a b c d e} H. Lux: On the knowledge of bromine chloride. In: Chem. Ber. 63, 1930, pp. 1156-1158, doi: 10.1002 / cber.19300630525 .
5. ↑ ^{a b c d} L. Kolditz: Inorganic Chemistry. Deutscher Verlag der Wissenschaften, Berlin 1983, p. 528.
6. ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Dipole Moments, pp. 9-51.
7. ^ P Lebeau: In: Compt. rend. Acad. Sciences. 143, 1906, p. 589.
8. ^ BJ Karsten: About the mutual behavior of the halogens, especially the chlorine-bromine and chlorine-iodine systems. In: Z. anorg. Chem. 53, 1907, pp. 365-392, doi: 10.1002 / zaac.19070530126 .
9. ^ ^{A b} V. Thomas, P Dupuis: In: Comptes Rendus Hebdomadaires des Seances de l'Academie des Sciences. 143, 1906, p. 282. Full text
10. ↑ M. Delepine, L Ville: In: Compt. rend. Acad. Science. 170, 1920, p. 1390.
11. ↑ GS Forbes, RM Fuoss: The Reaction Between Bromine and Chloride ion in Hydrochloric Acid. Bromine Chloride. In: J. Am. Chem. Soc. 49, 1927, pp. 142-156, doi: 10.1021 / ja01400a019 .
12. ^ S Barratt: In: Proc. Roy. Soc. London. 122, 1929, p. 582.
13. ↑ tayloredge.com: Lithium Battery Chemistry (PDF, English; 355 kB)
14. ↑ cdpr.ca.gov (English) ( Memento from June 1, 2010 in the Internet Archive ).