Dibortetrachloride

Structural formula
General
Surname	Dibortetrachloride
other names	Tetrachlorodiborane
Molecular formula	B 2 Cl 4
Brief description	colorless liquid
External identifiers / databases
CAS number 13701-67-2 PubChem 139548 Wikidata Q5272281
properties
Molar mass	163.43 g mol −1
Physical state	liquid
density	1.5 g cm −3 (0 ° C)
Melting point	−92.6 ° C
boiling point	65.5 ° 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 .

Dibortetrachloride is a chemical compound of boron from the group of chlorides .

Extraction and presentation

Dibortetrachloride can be obtained by reacting boron trichloride with mercury or copper in an electrical discharge.

${\displaystyle \mathrm {2\ BCl_{3}+2\ Hg\longrightarrow B_{2}Cl_{4}+Hg_{2}Cl_{2}} }$

${\displaystyle \mathrm {2\ BCl_{3}+2\ Cu\longrightarrow B_{2}Cl_{4}+2\ CuCl} }$

properties

Dibortetrachloride is a colorless liquid that dissolves in water to form boric acid and hydrochloric acid .

${\displaystyle \mathrm {B_{2}Cl_{4}+6\ H_{2}O\longrightarrow 2\ B(OH)_{3}+H_{2}+4\ HCl} }$

Like the other boron tetrahalides, it already decomposes at room temperature, the rate of decomposition increasing under the catalytic influence of the decomposition products.

${\displaystyle \mathrm {B_{2}Cl_{4}\longrightarrow 1/n(BCl)_{n}+BCl_{3}} }$

The connection ignites immediately in air.

${\displaystyle \mathrm {6\ B_{2}Cl_{4}+3\ O_{2}\longrightarrow 2\ B_{2}O_{3}+8\ BCl_{3}} }$

In the solid state it has an orthorhombic crystal structure with the space group Pbca (space group no. 61) . Dibortetrachloride forms adducts of the type B ₂ Cl ₄ · 2D with donors D (e.g. hydrogen sulfide) . It reacts with hydrogen to form dichloroborane .

use

Dibortetrachloride can be used to make organoboron compounds. Dibortetrafluoride can be obtained by reaction with antimony trifluoride .

${\displaystyle \mathrm {3\ B_{2}Cl_{4}+4\ SbF_{3}\longrightarrow 3\ B_{2}F_{4}+4\ SbCl_{3}} }$

Individual evidence

1. ↑ ^{a b c d e} Georg Brauer , with the collaboration of Marianne Baudler u. a. (Ed.): Handbook of Preparative Inorganic Chemistry . 3rd, revised edition. tape I . Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , pp. 799 .
2. ↑ ^{a b c d} Jean d'Ans, Ellen Lax, Roger Blachnik: Pocket book for chemists and physicists . Springer DE, 1998, ISBN 3-642-58842-5 , pp. 314 ( limited preview in Google Book search).
3. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
4. ^ ^{A b} A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 1033.
5. ^ Wiley-VCH: Ullmann's Fine Chemicals . John Wiley & Sons, 2013, ISBN 978-3-527-68357-4 , pp. 351 ( limited preview in Google Book Search).
6. ↑ Grant Urry, James Kerrigan, Theran D. Parsons, HI Schlesinger: Diboron Tetrachloride, B2Cl4, as a Reagent for the Synthesis of Organo-boron Compounds. I. The Reaction of Diboron Tetrachloride with Ethylene. In: Journal of the American Chemical Society. 76, 1954, pp. 5299-5301, doi : 10.1021 / ja01650a011 .
7. ^ AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 1033.