Chemistry:Tungstate

From HandWiki
Short description: Chemical compound containing an oxyanion or mixed oxide of tungsten
Chemical structure of the orthotungstate ion (WO2−
4)

In chemistry, a tungstate is a compound that contains an oxyanion of tungsten or is a mixed oxide containing tungsten. The simplest tungstate ion is WO2−
4, "orthotungstate".[1] Many other tungstates belong to a large group of polyatomic ions that are termed polyoxometalates, ("POMs"), and specifically termed isopolyoxometalates as they contain, along with oxygen and maybe hydrogen, only one other element. Almost all useful tungsten ores are tungstates.[2]

Structures

Orthotungstates feature tetrahedral W(VI) centres with short W–O distances of 1.79 Å. Structurally, they resemble sulfates. Six-coordinate, octahedral tungsten dominates in the polyoxotungstates. In these compounds, the W–O distances are elongated.[1]

Some examples of tungstate ions:[3]

  • HWO−
    4     (hydrogentungstate)[3]
  • polymeric W
    2    O2−
    7     ions of various structures in Na
    2    W
    2    O
    7    , Li
    2    W
    2    O
    7     and Ag
    2    W
    2    O
    7    [4]
  • [W
    7    O
    24    ]6−     (paratungstate A)[3]
  • [W
    10    O
    32    ]4−     (tungstate Y)[5]
  • [H
    2    W
    12    O
    42    ]10−     (paratungstate B) [3]
  • α-[H
    2    W
    12    O
    40    ]6−     (metatungstate)[5]
  • β-[H
    2    W
    12    O
    40    ]6−     (tungstate X)[5]

See the tungstates category for a list of tungstates.

Occurrence

Tungstates occur naturally with molybdates. Scheelite, the mineral calcium tungstate, often contains a small amount of molybdate. Wolframite is manganese and iron tungstate, and all these are valuable sources of tungsten. Powellite is a mineral form of calcium molybdate containing a small amount of tungstate.

Reactions

Solutions of tungstates, like those of molybdates, give intensely blue solutions of complex tungstate(V,VI) analogous to the molybdenum blues when reduced by most organic materials.[1]

Unlike chromate, tungstate is not a good oxidizer, but like chromate, solutions of tungstate condense to give the isopolytungstates upon acidification.

References

  1. ↑ 1.0 1.1 1.2 Egon Wiberg, Arnold Frederick Holleman (2001). Inorganic Chemistry. Elsevier. ISBN 0-12-352651-5. 
  2. ↑ Lassner, Erik; Schubert, Wolf-Dieter; Lüderitz, Eberhard; Wolf, Hans Uwe (2005). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a27_229. 
  3. ↑ 3.0 3.1 3.2 3.3 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. 
  4. ↑ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN:0-19-855370-6
  5. ↑ 5.0 5.1 5.2 Jon A. McCleverty, N. G. Connelly,Nomenclature of inorganic chemistry II: recommendations 2000, International Union of Pure and Applied Chemistry Commission on the Nomenclature of Inorganic Chemistry, Published by Royal Society of Chemistry, 2001, ISBN:0-85404-487-6



Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Tungstate&oldid=2599878"