Tellurate

The structure of metatellurate and orthotellurate

In chemistry tellurate is a compound containing an oxyanion of tellurium where tellurium has an oxidation number of +6. In the naming of inorganic compounds it is a suffix that indicates a polyatomic anion with a central tellurium atom.[1]

Tellurium oxyanions

Historically the name tellurate was only applied to oxyanions of tellurium with oxidation number +6, formally derived from telluric acid Te(OH)6, and the name tellurite referred to oxyanions of tellurium with oxidation number +4, formally derived from tellurous acid (HO)2TeO and these names are in common use. However tellurate and tellurite are often referred to as tellurate(VI) and tellurate(IV) respectively in line with IUPAC renaming recommendtaions.[1] The metatellurate ion is TeO2−
4 and the orthotellurate ion is TeO6−
6. Other oxyanions include pentaoxotellurate, TeO4−
5,[2] ditellurate, Te
2O8−
10[3] and polymeric anions with 6-coordinate tellurium such as (TeO4−
5)n.[4]

Metatellurates

The metatellurate ion TeO2−
4 is analogous to the sulfate ion, SO2−
4 and the selenate ion, SeO2−
4. Whereas many sulfates and selenates form isomorphous salts[5] the tetrahedral metatellurate ion is only found in a few compounds such as the tetraethylammonium salt NEt4TeO4.[6] Many compounds with a stoichiometry that suggests the presence of a metatellurate ion actually contain polymeric anions containing 6-coordinate tellurium(VI), for example sodium tellurate, Na2TeO4 which contains octahedral tellurium centers sharing edges.[7]

TeO2−
4 → TeO2−
3 + 1⁄2 O2      (E0 = −1.042 V)

The E0 or standard reduction potential value is significant as it gives an indication of the strength of the tellurate ion as an oxidizing agent.[8]

Orthotellurates

Compounds containing the octahedral TeO6−
6 anion are known, these include Ag6TeO6, Na6TeO6 and Hg3TeO6.[9] There are also hydroxyoxotellurates, containing protonated TeO6−
6, such as (NH4)2TeO2(OH)4 (sometimes written as NH4TeO4·2H2O) which contains the octahedral TeO
2(OH)2−
4 ion.[10]

TeO4−
5 ion

The compound Cs2K2TeO5 contains TeO4−
5 ions which are trigonal bipyramidal.[2] The compound Rb6Te2O9 contains both TeO4−
5 and TeO2−
4 anions.[11] Other compounds whose stoichiometry suggests the presence of TeO4−
5 may contain either the dimeric Te
2O8−
10 made up of two edge-sharing {TeO6} as in Li4TeO5[3] and Ag4TeO5[12] or corner-sharing {TeO6} octahedra as in Hg2TeO5.[4]

Polymeric tellurate ions

The dimeric Te
2O8−
10 made up of two edge sharing {TeO6} octahedra is found in the compound, Li4TeO5.[3] A similar hydroxy-oxy anion, Te2O6(OH)4 is found in sodium potassium ditellurate(VI) hexahydrate,Na0.5K3.5Te2O6(OH)4·6H2O which contains pairs of edge sharing octahedra.[13] Polymeric chain anions consisting of corner-shared {TeO6} octahedra (TeO5)4n−
n are found, for example in Li4TeO5.[3]

Aqueous chemistry

In aqueous solution tellurate ions are 6 coordinate. In neutral conditions the pentahydrogen orthotellurate ion, H
5TeO−
6, is the most common; in basic conditions, the tetrahydrogen orthotellurate ion, H
4TeO2−
6, and in acid conditions, orthotelluric acid, Te(OH)6 or H6TeO6 is formed.[8]

Structural comparisons with oxyanions of sulfur and selenium

Sulfur(VI) oxyanions have a coordination number of 4 and in addition to the tetrahedral sulfate ion, SO2−
4, the pyrosulfate, S
2O2−
7, trisulfate, S
3O2−
10 and pentasulfate S
5O2−
16 ions all contain 4-coordinate sulfur and are built from corner-shared {SO4} tetrahedra.[14] Selenate compounds include many examples of four coordinate selenium, principally the tetrahedral SeO2−
4 ion and the pyroselenate ion, S
2O2−
7 which has a similar structure to the pyrosulfate ion.[15] Unlike sulfur there are examples of a 5-coordinate selenium oxyanion, SeO4−
5 and one example of SeO6−
6.[16][17][18]

NMR spectroscopy

Tellurium has two NMR active nuclei, 123Te and 125Te. 123Te has an abundance of 0.9% and a nuclear spin (I) of 1⁄2. 125Te has an abundance of 7% and an equivalent nuclear spin.[19] 125Te is more commonly performed because it has a higher sensitivity.[20] The metatellurate anion has a chemical shift around 610 ppm when analyzed using 125Te NMR at 25 °C at a frequency of 94.735 MHz and referenced externally against aqueous 1.0 M telluric acid.[6]

The tellurate suffix in the naming of inorganic compounds

Following the IUPAC Red Book(2005)[1] some examples are:

References

  1. 1 2 3 Nomenclature of Inorganic Chemistry IUPAC Recommendations 2005 – Full text (PDF)
  2. 1 2 Untenecker, H.; Hoppe, R. (1986). "Die koordinationszahl 5 bei telluraten: Cs2K2[TeO5]". Journal of the Less Common Metals 124 (1-2): 29–40. doi:10.1016/0022-5088(86)90474-1. ISSN 0022-5088.
  3. 1 2 3 4 Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  4. 1 2 Weil, Matthias (2003). "Preparation, Thermal Behaviour and Crystal Structure of the Basic Mercury(II) Tetraoxotellurate(VI), Hg2TeO5, and Redetermination of the Crystal Structure of Mercury(II) Orthotellurate(VI), Hg3TeO6". Zeitschrift für anorganische und allgemeine Chemie 629 (4): 653–657. doi:10.1002/zaac.200390111. ISSN 0044-2313.
  5. ↑ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, p. 531, ISBN 0-471-19957-5
  6. 1 2 Konaka, Saki; Ozawa, Yoshiki; Yagasaki, Atsushi (2008). "Tetrahedral Tellurate". Inorganic Chemistry 47 (4): 1244–1245. doi:10.1021/ic701578p. ISSN 0020-1669.
  7. ↑ Kratochvíl, B.; Jenšovský, L. (1977). "The crystal structure of sodium metatellurate". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 33 (8): 2596–2598. doi:10.1107/S0567740877008978. ISSN 0567-7408.
  8. 1 2 Frost, Ray L. (2009). "Tlapallite H6(Ca,Pb)2(Cu,Zn)3SO4(TeO3)4TeO6, a multi-anion mineral: A Raman spectroscopic study". Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy 72 (4): 903–906. doi:10.1016/j.saa.2008.12.008. ISSN 1386-1425.
  9. ↑ Holleman, A. F.; Wiberg, E. (2001), Inorganic Chemistry, San Diego: Academic Press, p. 593, ISBN 0-12-352651-5
  10. ↑ Johansson, G. B.; Lindqvist, O.; Moret, J. (1979). "Diammonium tellurium(VI) dioxide tetrahydroxide". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 35 (7): 1684–1686. doi:10.1107/S056774087900741X. ISSN 0567-7408.
  11. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 782. ISBN 0-08-037941-9.
  12. ↑ Weil, Matthias (2007). "New Silver Tellurates – The Crystal Structures of a Third Modification of Ag2Te2O6 and of Ag4TeO5". Zeitschrift für anorganische und allgemeine Chemie 633 (8): 1217–1222. doi:10.1002/zaac.200700106. ISSN 0044-2313.
  13. ↑ Kratochvíl, B.; Podlahová, J.; Jenšovský, L. (1978). "Sodium potassium ditellurate(VI) hexahydrate". Acta Crystallographica Section B 34 (1): 256–258. doi:10.1107/S056774087800271X. ISSN 0567-7408.
  14. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 712. ISBN 0-08-037941-9.
  15. ↑ Paetzold, R.; Amoulong, H.; Růžička, A. (1965). "Untersuchungen an Selen-Sauerstoff-Verbindungen. XXVI. Schwingungsspektrum und Kraftkonstanten des Diselenations". Zeitschrift für anorganische und allgemeine Chemie 336 (5-6): 278–285. doi:10.1002/zaac.19653360508. ISSN 0044-2313.
  16. ↑ Haas, Helmut; Jansen, Martin (2000). "Octahedral SeO6−
    6     and Square-Pyramidal SeO4−
    5    , Two New Oxoselenate Anions". Angewandte Chemie 39 (23): 4362–4364. doi:10.1002/1521-3773(20001201)39:23<4362::AID-ANIE4362>3.0.CO;2-S. ISSN 1433-7851.
  17. ↑ Orosel, Denis; Dinnebier, Robert; Jansen, Martin (2006). "High-Pressure Synthesis and Structure Determination of K6(SeO4)(SeO5), the First Potassium Orthoselenate(VI)". Inorganic Chemistry 45 (26): 10947–10950. doi:10.1021/ic061548v. ISSN 0020-1669.
  18. ↑ Haas, H.; Jansen, M. (2001). "Na4SeO5, ein neues Pentaoxoselenat(VI) – Synthese, Charakterisierung und Vergleich mit isotypem Na4MoO5". Zeitschrift für anorganische und allgemeine Chemie 627 (4): 755–760. doi:10.1002/1521-3749(200104)627:4<755::AID-ZAAC755>3.0.CO;2-L. ISSN 0044-2313.
  19. ↑ Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. ISBN 978-0131755536.
  20. ↑ Drago, R. S. Physical Methods for Chemists 2nd ed.; Surfside Scientific Publishers: Gainesville, FL 1992.
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