Vanadyl sulfate

Crystal structure
	Vanadyl sulfate pentahydrate ; __ V __ S __ O
General
Surname	Vanadyl sulfate
other names	Vanadium (IV) oxide sulfate; Vanadium oxysulfate; Vanadium (IV) oxide sulfate; Vanadyl sulfate;
Ratio formula	VOSO 4 ; VOSO 4 5 H 2 O (pentahydrate);
Brief description	green solid (anhydrous); blue odorless solid (pentahydrate);
External identifiers / databases
EC number	248-652-7
ECHA InfoCard	100.044.214
PubChem	34007
ChemSpider	31347
Wikidata	Q413634
properties
Molar mass	163.00 g mol −1
Physical state	firmly
density	1.09 g cm −3
Melting point	105 ° C
solubility	practically insoluble in water (anhydrous); easily soluble in water (pentahydrate);
safety instructions
H and P phrases	H: 290-302-315-319-361-372-411
	P: 234-260-273-281-301 + 330 + 331-302 + 352-305 + 351 + 338
Toxicological data	448 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 .

Vanadyl sulfate , VOSO ₄ , is an inorganic compound of vanadium .

Occurrence

Like most water-soluble sulfates, it is very rarely found in nature. The anhydrous form is pauflerite , a mineral of fumarole origin. The hydrates are also very rare; Hexahydrate ( Stanleyit ), Pentahydrate ( Minasragrit , Orthominasragrit and Anorthominasragrit ) and trihydrate ( Bobjonesit ).

presentation

Vanadyl sulfate is usually prepared by reducing vanadium (V) oxide with sulfur dioxide :

{\ displaystyle \ mathrm {V_ {2} O_ {5} +7 \ H_ {2} O + SO_ {2} + H_ {2} SO_ {4} \ longrightarrow}}

{\ displaystyle \ mathrm {2 \ [V (O) (H_ {2} O) _ {4}] SO_ {4}}}

The anhydrous compound can be obtained by boiling the vanadium (V) oxide in concentrated sulfuric acid for several hours :

{\ displaystyle {\ ce {2 V2O5 + 4 H2SO4 -> 4 VOSO4 + 4 H2O + O2}}}

properties

Vanadyl sulfate

The highly hygroscopic , blue solid (pentahydrate) is one of the most common sources of vanadium in the laboratory. It contains the vanadyl ion , VO ²⁺ , which has been called the “most stable diatomic ion”.

In aqueous solution, the salt crystallizes as a pentahydrate , the fifth water is not bound to the metal. Seen as a complex , it has an octahedral structure, with oxygen, four waters and a sulfate as ligands. The V = O bond length is 160 pm , which is 50 pm shorter than the V – OH ₂ bonds. The sulfate ion dissociates very quickly in solution.

The pentahydrate and the trihydrate have a monoclinic crystal structure with the space group P 2 ₁ / a (space group no. 14, position 3) . Template: room group / 14.3

In acidic solution, the oxidation of vanadyl sulfate gives yellow colored vanadyl (V) derivatives. A reduction, e.g. B. by zinc , gives vanadium (III) - and vanadium (II) - derivatives, which are characteristic green and purple.

use

Vanadyl sulfate is usually a common starting material for other vanadyl derivatives, such as vanadium (IV) oxy (acetylacetonate) :

{\ displaystyle \ mathrm {[V (O) (H_ {2} O) _ {4}] SO_ {4} + C_ {5} H_ {8} O_ {2} + Na_ {2} CO_ {3} \ longrightarrow}}

{\ displaystyle \ mathrm {[V (O) (C_ {5} H_ {7} O_ {2}) _ {2}] + Na_ {2} SO_ {4} +4 \ H_ {2} O + CO_ { 2}}}

Vanadyl sulfate is an intermediate in the extraction of vanadium from petroleum residues, a major commercial source of vanadium.

Vanadyl sulfate is found in some dietary supplements , especially abroad, for example in the USA . In the bodybuilding sector in particular, helpful effects of vanadyl sulfate are advertised, but no verifiable effect could be determined. Vanadyl compounds are said to mimic the effect of insulin, the mode of action is described similar to that of chromium picolinate . Vanadyl sulfate is not permitted as a mineral in Germany .

swell

Norman Neill Greenwood, Alan Earnshaw: Chemistry of the elements . Pergamon Press, Oxford 1984, ISBN 978-0-08-022056-7 , pp. 1157 .
Günter Bauer, Volker Güther, Hans Hess, Andreas Otto, Oskar Roidl, Heinz Roller, Siegfried Sattelberger: Vanadium and vanadium compounds . In: Ullman's Encyclopedia of Industrial Chemistry . A27. Wiley-VCH, Weinheim 2002, p. 367-386 ( PDF ).
Burl E. Bryant, W. Conard Fernelius, Daryle H. Busch, R. Carl Stoufer, Wilmer Stratton: Vanadium (IV) Oxy (acetylacetonate) . In: Inorganic Syntheses . 1957, p. 113-116 , doi : 10.1002 / 9780470132364.ch30 .

Individual evidence

↑ ^a ^b ^c ^d Georg Brauer: Vandin (IV) oxysulfate (vanadyl sulfate) . In: Handbook of Preparative Inorganic Chemistry . Ferdinand Enke Verlag, Stuttgart 1954, p. 965-966 .
↑ ^a ^b ^c ^d ^e ^f ^g ^h Entry on vanadium (IV) oxide sulphate in the GESTIS substance database of the IFA , accessed on February 1, 2016(JavaScript required) .
↑ ML Smith, J. Marinenko: A reexamination of minasragrite . In: American Mineralogist . tape 58 , 1973, p. 531-534 ( online [PDF]).
^ ^A ^b Chemisches und Veterinäruntersuchungsamt Karlsruhe: Prohibited substances in food supplements ( Memento of October 24, 2007 in the Internet Archive )
↑ Pharmaceutical newspaper online: Beware of the prohormone trap , 10/2004.

[Brauer-1] Georg Brauer: Vandin (IV) oxysulfate (vanadyl sulfate) . In: Handbook of Preparative Inorganic Chemistry . Ferdinand Enke Verlag, Stuttgart 1954, p. 965-966 .

[GESTIS-2] ↑ ^a ^b ^c ^d ^e ^f ^g ^h Entry on vanadium (IV) oxide sulphate in the GESTIS substance database of the IFA , accessed on February 1, 2016(JavaScript required) .

[3] ML Smith, J. Marinenko: A reexamination of minasragrite . In: American Mineralogist . tape 58 , 1973, p. 531-534 ( online [PDF]).

[cvua-4] A ^b Chemisches und Veterinäruntersuchungsamt Karlsruhe: Prohibited substances in food supplements ( Memento of October 24, 2007 in the Internet Archive )

[5] Pharmaceutical newspaper online: Beware of the prohormone trap , 10/2004.