Dysprosium(II) chloride (DyCl2), also known as dysprosium dichloride, is an ionic chemical compound of dysprosium and chlorine. This salt is a reduced compound, as the normal oxidation state of dysprosium in dysprosium compounds is +3.
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| IUPAC names
Dysprosium(II) chloride
Dysprosium dichloride | |
| Identifiers | |
3D model (JSmol)
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| DyCl2 | |
| Molar mass | 233.406 g/mol |
| Related compounds | |
Other cations
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NdCl2, SmCl2, EuCl2, TmCl2, YbCl2 |
Related compounds
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Dysprosium(III) chloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Dysprosium dichloride is glossy black in appearance. The salt is damaged by oxidation on exposure to air. It is an electrical insulator.[2]
The structure is the same as for strontium bromide, ytterbium dichloride, and terbium dichloride. There are two forms. The low temperature form is below 652 °C. It is orthorhombic with unit cell dimensions a=6.69, b=6.76, and c=7.06 Å.[3]
Preparation
editDysprosium dichloride can be prepared by heating molten dysprosium trichloride with dysprosium metal, and rapidly quenching. Molybdenum, niobium or tantalum crucibles are required to avoid alloy formation with the dysprosium.[4]
Reactions
editDysprosium dichloride is capable of reducing titanium dichloride to titanium metal in a potassium chloride, sodium chloride flux.[5]
- Ti2+ + 2Dy2+ → Ti (solid) + 2Dy3+
Related
editA ternary dysprosium(II) chloride compound is known with lithium: LiDy2Cl5. This is produced by heating lithium metal and dysprosium trichloride together at 700 °C. This compound is also black. The crystal system of LiDy2Cl5 is monoclinic with space group C2/c 4 formulae per unit cell which has dimensions ; a = 16.45.6(; b = 6.692; and c = 7.267; with β = 95.79°.[6]
References
edit- ^ "Dysprosium dichloride". webbook.nist.gov.
- ^ Macintyre, Jane E. (1992-07-23). Dictionary of Inorganic Compounds. CRC Press. p. 2867. ISBN 978-0-412-30120-9.
- ^ Corbett, John D.; McCollum, Bill C. (May 1966). "Rare Earth Metal-Metal Halide Systems. IX. The Dysprosium-Dysprosium(III) Chloride System and the Preparation of Dysprosium(II) Chloride". Inorganic Chemistry. 5 (5): 938–940. doi:10.1021/ic50039a050.
- ^ Advances in Inorganic Chemistry and Radiochemistry. Academic Press. 1977-09-01. p. 8. ISBN 978-0-08-057869-9.
- ^ Yasuda, Kouji; Saegusa, Kunio; Okabe, Toru H. (January 2011). "Aluminum Subhalide as a Reductant for Metallothermic Reduction". High Temperature Materials and Processes. 30 (4–5): 411. Bibcode:2011HTMP...30..411Y. doi:10.1515/htmp.2011.063.
- ^ Meyer, Gerd (September 1983). "Reduced ternary rare earth halides: State of the art". Journal of the Less Common Metals. 93 (2): 371–380. doi:10.1016/0022-5088(83)90190-X.