Names | |
---|---|
IUPAC name
europium(II) sulfide
| |
Identifiers | |
3D model (JSmol)
|
|
ECHA InfoCard | 100.031.498 |
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 | |
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]
YouTube Encyclopedic
-
1/4Views:80 63863515 4913 841
-
Make Europium and Dysprosium Nitrate salts.
-
Europium
-
How to Write the Formula for Iron (II) nitride
-
How to Write the Formula for Chromium (II) nitride
Transcription
Greetings fellow nerds. In upcoming videos we're going to need the europium and dysprosium nitrate salts, more specifically the pentahydrate forms. We've given this procedure it's own separate video to make the upcoming videos shorter and more to the point. Pure europium and dysprosium metal can be purchased from online element dealers. There very popular for element collectors, and a few will sell directly to individuals. This makes europium and dysprosium nitrate very accessible to non-scientists. Look in the video description for the links. Alright, let's first start with europium nitrate. Here we have a 2.5 gram sample of pure europium metal. Europium metal is highly reactive even toward air, so when you buy it the europium will come stored in mineral oil. Carefully take it out with tweezers and wash it thoroughly in some toluene to get rid of the mineral oil. Hold it in the air for a few minutes to dry it out. Then place it in a beaker. As you can see, it's already starting to react with the air to produce that yellowish white oxide layer. Now carefully pour in a total of 10 mL of pure distilled water. As you can see, europium metal is highly reactive toward water, about the same level as calcium. As it reacts, it produces europium hydroxide that covers the metal and slows down the reaction. When the reaction seems to have stopped, carefully add in a total of 10 mL of concentrated 15.6 molar nitric acid in small portions. Let the mixture react until it's just bits of dust left over. Now carefully heat the mixture until it boils and completely dissolves the metal. Now we have a pure solution of europium nitrate with excess nitric acid. We'll make this into a powder in a moment. But now, let's do dysprosium nitrate. Here is a 5 gram sample of dysprosium metal. Place it in the beaker and then add 20 mL of pure distilled water. As you can see, dysprosium is much less reactive than europium. To get it going, directly add 20 mL of concentrated 15.6 molar nitric acid. As it reacts it will produce nitrogen dioxide. Once again, let it react until it's just a suspension of metal particles. Then boil it until it completely dissolves. Now you have a yellow solution of pure dysprosium nitrate with nitric acid. Now place both nitrates into the desiccator bag we made in a previous video. You cannot simply boil them down because these nitrates are so sensitive that they'll decompose if heated to dryness. You also cannot simply leave them out to evaporate because they're extremely hygroscopic and almost never crystallize out of solution. Alright, after a few weeks in the bag with the occasional mash up to expose any pockets of moisture, take out the nitrates. Make sure they're dry enough by crushing them and seeing if they crumble to a powder rather than a paste. If they are dry, transfer them into vials with air tight caps. Remember to clearly label the vials. After years of being a sloppy chemist I learned this important lesson the hard way. Anyway, here we have our finished rare-earth europium and dysprosium nitrates. We're specifically going to use them for their metal component in some very cool upcoming videos so please subscribe, rate and comment.
Structure
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
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
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
- ^ 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. doi:10.1073/pnas.1919753117. ISSN 0027-8424. PMC 7183215. PMID 32253317.