Europium(II) sulfide
| |
| Names | |
|---|---|
| IUPAC name
europium(II) sulfide
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.031.498 |
| EC Number |
|
PubChem CID
|
|
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| EuS | |
| Molar mass | 184.03 g/mol |
| Appearance | black powder |
| Melting point | 2,250 °C (4,080 °F; 2,520 K) |
| +25,730;·10−6 cm3/mol | |
| Hazards | |
| GHS labelling:[1] | |
| |
| Warning | |
| H228 | |
| P210, P240, P241, P280, P370+P378 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Europium(II) sulfide is the inorganic compound with the chemical formula EuS. It is a black, air-stable powder. Europium possesses an oxidation state of +II in europium sulfide, whereas the lanthanides exhibit a typical oxidation state of +III.[1] Its Curie temperature (Tc) is 16.6 K. Below this temperature EuS behaves like a ferromagnetic compound, and above it exhibits simple paramagnetic properties.[2] EuS is stable up to 500 °C in air, when it begins to show signs of oxidation. In an inert environment it decomposes at 1470 °C.[3]
Structure
[edit]EuS crystallizes in face-centered cubic (FCC) crystal lattice with the rock salt structure. Both europium and sulfur have octahedral coordination geometry with a coordination number of six.[4][5] The Eu-S bond lengths are 2.41 Å.
Preparation
[edit]In the preparation of EuS, powdered europium(III) oxide (Eu2O3) is treated with hydrogen sulfide (H2S) at 1150 °C. The crude EuS product is purified by heating at 900 °C under vacuum to remove excess sulfur.[4][3]
- Eu2O3 + 3 H2S → 2 EuS + 3 H2O + S
EuS has additionally been synthesized from europium dichloride (EuCl2), however, such products tend to be contaminated by chloride.[4]
Research
[edit]In the past few decades, a new interest has been exhibited in the synthesis of EuS, as well as its oxygen analog EuO, because of their potential as laser window materials, insulating ferromagnets, ferromagnetic semiconductors, and magnetoresistant, optomagnetic, and luminescent materials.[3][2] EuS was used in an experiment providing evidence of Majorana fermions relevant to quantum computing and the production of qubits.[6]
References
[edit]- ^ C. Housecroft. Inorganic Chemistry. 3rd. Essex, England: Pearson Education Limited, 2008. Print. ISBN 0-13-175553-6
- ^ a b Zhao, Fei; Sun, Hao-Ling; Su, Gang; Gao, Song (2006). "Synthesis and Size-Dependent Magnetic Properties of Monodisperse EuS Nanocrystals". Small. 2 (2). Wiley: 244–248. doi:10.1002/smll.200500294. ISSN 1613-6810. PMID 17193029.
- ^ a b c Ananth, K.P.; Gielisse, P.J.; Rockett, T.J. (1974). "Synthesis and characterization of europium sulfide". Materials Research Bulletin. 9 (9). Elsevier BV: 1167–1171. doi:10.1016/0025-5408(74)90033-6. ISSN 0025-5408.
- ^ a b c Archer, R. D. Mitchel, W. N. Inorganic Syntheses, Europium (II) Sulfide. 1967, volume 10, 77-79. doi:10.1002/9780470132418
- ^ Wells A.F. Structural Inorganic Chemistry. 5th. London, England: Oxford University Press, 1984. Print. ISBN 0-19-855370-6
- ^ Manna, Sujit; Wei, Peng; Xie, Yingming; Law, Kam Tuen; Lee, Patrick A.; Moodera, Jagadeesh S. (2020-04-06). "Signature of a pair of Majorana zero modes in superconducting gold surface states". Proceedings of the National Academy of Sciences. 117 (16): 8775–8782. arXiv:1911.03802. Bibcode:2020PNAS..117.8775M. doi:10.1073/pnas.1919753117. ISSN 0027-8424. PMC 7183215. PMID 32253317.