3D model (JSmol)
|Molar mass||186.11 g/mol|
|Density||2.91 g/cm3, solid|
|Melting point||1,775 °C (3,227 °F; 2,048 K)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
The crystal structure of Sc2S3 is closely related to that of sodium chloride, in that it is based on a cubic 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, orthorhombic unit cell belonging to the space group Fddd.
Metal sulfides are usually prepared by heating mixtures of the two elements, but in the case of scandium, this method yields scandium monosulfide, ScS. Sc2S3 can be prepared by heating scandium(III) oxide under flowing hydrogen sulfide in a graphite crucible to 1550 °C or above for 2–3 hours. The crude product is then purified by chemical vapor transport at 950 °C using iodine as the transport agent.
- Sc2O3 + 3H2S → Sc2S3 + 3H2O
- 2 ScCl3 + 3 H2S → Sc2S3 + 6 HCl
- Dismukes, J. P.; White, J. G. (1964). "The Preparation, Properties, and Crystal Structures of Some Scandium Sulfides in the Range Sc2S3-ScS". Inorg. Chem. 3 (9): 1220–1228. doi:10.1021/ic50019a004.
- Klemm, W.; Meisel, K.; v. Vogel, H. U. (1930). "Über die Sulfide der seltenen Erden (Sulfides of the rare earths)". Zeitschrift fuer Anorganische und Allgemeine Chemie. 190: 123–144. doi:10.1002/zaac.19301900113.CS1 maint: Uses authors parameter (link)