-sulfide-xtal-1964-unit-cell-CM-3D-balls.png) | |
| Names | |
|---|---|
| Other names scandium sesquisulfide | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider | |
| ECHA InfoCard | 100.032.097 |
| EC Number |
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| |
| |
| Properties | |
| Sc2S3 | |
| Molar mass | 186.11 g/mol |
| Appearance | yellow crystals |
| Density | 2.91 g/cm3, solid |
| Melting point | 1,775 °C (3,227 °F; 2,048 K) |
| Structure | |
| orthorhombic | |
| Related compounds | |
Otheranions | Scandium oxide |
Othercations | Yttrium(III) sulfide |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Scandium(III) sulfide is achemical compound ofscandium andsulfur with thechemical formulaSc2S3. It is a yellow solid.
Thecrystal structure of Sc2S3 is closely related to that ofsodium chloride, in that it is based on acubic close packed array of anions. Whereas NaCl has all the octahedral interstices in the anion lattice occupied by cations, Sc2S3 has one third of them vacant. The vacancies are ordered, but in a very complicated pattern, leading to a large, orthorhombicunit cell belonging to thespace group Fddd.[1]
Metal sulfides are usually prepared by heating mixtures of the two elements, but in the case of scandium, this method yieldsscandium monosulfide, ScS. Sc2S3 can be prepared by heatingscandium(III) oxide under flowinghydrogen sulfide in agraphitecrucible to 1550 °C or above for 2–3 hours. The crude product is then purified bychemical vapor transport at 950 °C usingiodine as the transport agent.[1]
Scandium(III) sulfide can be prepared by reactingscandium(III) chloride with dryhydrogen sulfide at elevated temperature:[2]
Above 1100 °C, Sc2S3 loses sulfur, formingnonstoichiometric compounds such as Sc1.37S2.[1]
