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Scandium oxide

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Scandium(III) oxide

__ Sc3 __ O2−
Names
IUPAC name
Scandium(III) oxide
Other names
Scandia, scandium sesquioxide
Identifiers
3D model (JSmol)
ECHA InfoCard 100.031.844 Edit this at Wikidata
UNII
  • InChI=1S/3O.2Sc
  • O=[Sc]O[Sc]=O
Properties
Sc2O3
Molar mass 137.910 g/mol
Appearance White powder
Density 3.86 g/cm3
Melting point 2,485 °C (4,505 °F; 2,758 K)
insoluble in water
Solubility soluble in hot acids (reacts)
Structure[1]
Bixbyite
Ia3 (No. 206)
a = 985 pm
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
Related compounds
Other anions
 Scandium(III) sulfide
Other cations
 Yttrium(III) oxide
Lutetium(III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Scandium(III) oxide or scandia is a inorganic compound with formula Sc2O3. It is one of several oxides of rare earth elements with a high melting point. 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

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

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

Production

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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 predominantly produced as a by-product from the extraction of other elements.

Reactions

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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 (but like lutetium oxide), for example forming K3Sc(OH)6 with KOH. In this, scandium oxide shows more similarity with aluminium oxide.

Natural occurrence

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Natural scandia, although impure, occurs as mineral kangite.[6]

References

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  1. ^ a b 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.
  2. ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  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"]
  6. ^ Mindat, http://www.mindat.org/min-42879.html
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