Vanadium (IV) chloride

Structural formula
General
Surname	Vanadium (IV) chloride
other names	Vanadium tetrachloride; Vanadium (IV) chloride; Vanadium tetrachloride;
Molecular formula	VCl 4
Brief description	reddish-brown liquid with a pungent odor
External identifiers / databases
EC number	231-561-1
ECHA InfoCard	100.028.692
PubChem	24273
ChemSpider	22693
Wikidata	Q421255
properties
Molar mass	192.75 g mol −1
Physical state	liquid
density	1.82 g cm −3
Melting point	−28 ° C
boiling point	154 ° C
Vapor pressure	7.9 h Pa (20 ° C)
solubility	decomposes in water with violent reaction
safety instructions
H and P phrases	H: 301 + 311 + 331-314
	EUH: 014
	P: 261-280-301 + 310-305 + 351 + 338-310
Toxicological data	160 mg kg −1 ( LD 50 , rat , oral )
	As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Vanadium (IV) chloride is a chemical compound from the group of chlorides . It is in the form of an unstable, non-flammable, reddish-brown liquid with a pungent odor. When exposed to light or humidity, it decomposes with the formation of chlorine gas or hydrogen chloride .

Extraction and presentation

Vanadium (IV) chloride is by chlorination of the vanadium extracted at about 300-350 ° C.

{\ displaystyle \ mathrm {V + 2 \ Cl_ {2} \ longrightarrow VCl_ {4}}}

properties

Vanadium (IV) chloride is a dark red-brown, viscous liquid that smokes in air. Hydrolysis takes place with water (blue solution). It is soluble in concentrated hydrochloric acid (brown solution) and ether (deep red solution). Vanadium (IV) chloride is a powerful oxidizing agent .

Vanadium (IV) chloride slowly releases chlorine at room temperature as it disproportionates into the trichloride :

{\ displaystyle \ mathrm {2 \ VCl_ {4} \ longrightarrow 2 \ VCl_ {3} + Cl_ {2}}}

This can lead to the rupture of tightly closed vessels. Solutions can be stored in carbon tetrachloride without the risk of decomposition , from which it can be obtained in pure form by fractionation if necessary .

use

Vanadium (IV) chloride is used for the production of other vanadium compounds, as well as in organic syntheses and as a catalyst in the polymerisation of alkenes . For example, for the coupling of phenols :

{\ displaystyle \ mathrm {2 \ C_ {6} H_ {5} OH + 2 \ VCl_ {4} \ longrightarrow HOC_ {6} H_ {4} {-} C_ {6} H_ {4} OH + 2 \ VCl_ {3} +2 \ HCl}}

safety instructions

Vanadium (IV) chloride decomposes in water with violent reaction. It is classified as a carcinogen and germ cell mutagenic category 2.

Individual evidence

↑ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ Entry on vanadium (IV) chloride in the GESTIS substance database of the IFA , accessed on July 23, 2016(JavaScript required) .
↑ ^a ^b ^c Georg Brauer (Ed.) U. a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume III, Ferdinand Enke, Stuttgart 1981, ISBN 3-432-87823-0 , p. 1412.
^ AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 , p. 1548.

[GESTIS-1] ↑ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ Entry on vanadium (IV) chloride in the GESTIS substance database of the IFA , accessed on July 23, 2016(JavaScript required) .

[brauer-2] Georg Brauer (Ed.) U. a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume III, Ferdinand Enke, Stuttgart 1981, ISBN 3-432-87823-0 , p. 1412.

[howi-3] AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 , p. 1548.