Scandium oxide

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Scandium(III) oxide
Kristallstruktur Lanthanoid-C-Typ.png
__ Sc3+ __ O2−
Identifiers
CAS number 12060-08-1 YesY
PubChem 4583683
Jmol-3D images Image 1
Properties
Molecular formula Sc2O3
Molar mass 137.910 g/mol
Density 3.86 g/cm3
Melting point 2485 °C
Solubility in water insoluble in water
Solubility soluble in hot acids (reacts)
Hazards
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Scandium(III) oxide, Sc2O3, or scandia, is a high melting rare earth oxide. It is used in the preparation of other scandium compounds as well as in high-temperature systems (for its resistance to heat and thermal shock), electronic ceramics, and glass composition (as a helper material).

Structure and physical properties[edit]

Scandium(III) oxide adopts a cubic crystal structure (point group: tetrahedral (Th), space group: Ia3) containing 6-coordinate metal centres.[1] Powder diffraction analysis shows Sc-O bond distances of 2.159-2.071Å.[2]

Scandium Oxide is an insulator with a band gap of 6.0 eV.[3]

Production[edit]

Scandium oxide is the primary form of refined scandium produced by the mining industry. Scandium-rich ores, such as thortveitite (Sc,Y)2(Si2O7) and kolbeckite ScPO4·2H2O are rare, however trace amounts of scandium are present in many other minerals. Scandium oxide is therefore predominately produced as a by-product from the extraction of other elements.

Reactions[edit]

Scandium oxide is the primary form of refined scandium produced by the mining industry, making it the start point for all scandium chemistry.

Scandium oxide reacts with most acids upon heating, to produce the expected hydrated product. For example, heating in excess aqueous HCl produces hydrated ScCl3·nH2O. This can be rendered anhydrous by evaporation to dryness in the presence of NH4Cl, with the mixture then being purified by removal of NH4Cl by sublimation at 300-500°C.[4] The presence of NH4Cl is required, as the hydrated ScCl3·nH2O would otherwise form a mixed oxychloride upon drying.

Sc2O3 + 6 HCl + x H2O → 2 ScCl3·nH2O + 3 H2O
ScCl3·nH2O + n NH4Cl → ScCl3 + n H2O + n NH4Cl

Likewise, it is converted into hydrated scandium(III) triflate (Sc(OTf)3·nH2O) by a reaction with triflic acid.[5]

Metallic scandium is produced industrially by the reduction of scandium oxide; this proceeds via conversion to scandium fluoride followed by a reduction with metallic calcium. This process is in some ways similar to the Kroll process for the production of metallic titanium.

Scandium oxide forms scandate salts with alkalis, unlike its higher homologues yttrium oxide and lanthanum oxide, for example forming K3Sc(OH)6 with KOH. In this, scandium shows more similarity with aluminium oxide.

References[edit]

  1. ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  2. ^ Knop, Osvald; Hartley, Jean M. (15 April 1968). "Refinement of the crystal structure of scandium oxide". Canadian Journal of Chemistry 46 (8): 1446–1450. doi:10.1139/v68-236. 
  3. ^ Emeline, A. V.; Kataeva, G. V.; Ryabchuk, V. K.; Serpone, N. (1 October 1999). "Photostimulated Generation of Defects and Surface Reactions on a Series of Wide Band Gap Metal-Oxide Solids". The Journal of Physical Chemistry B 103 (43): 9190–9199. doi:10.1021/jp990664z. 
  4. ^ Stotz, Robert W.; Melson, Gordon A. (1 July 1972). "Preparation and mechanism of formation of anhydrous scandium(III) chloride and bromide". Inorganic Chemistry 11 (7): 1720–1721. doi:10.1021/ic50113a058. 
  5. ^ McCleverty, J.A. and Meyer, T.J., Comprehensive Coordination Chemistry II, 2003, Elsevier Science, ISBN 0-08-043748-6, Vol. 3, p. 99 ["Refluxing scandium oxide with triflic acid leads to the isolation of hydrated scandium triflate"]