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Dysprosium(III) chloride
| Dysprosium(III) chloride hexahydrate | |
| IUPAC name Dysprosium(III) chloride | |
| General | |
|---|---|
| Molecular formula | DyCl3 |
| Molecular weight | 268.86 amu (anhydrous) |
| Appearance | white or yellow solid (anhydrous)
white to pale yellow crystalline solid (hexahydrate) |
| CAS number | [10025-74-8] (anhydrous)
[15059-52-6] (hexahydrate) |
| MSDS | Dysprosium(III) chloride MSDS |
| Other names | |
| |
| Bulk Properties | |
| Density | 3.67 g/cm3 (anhydrous) |
| Solubility | water: soluble |
| Melting point | 647 °C (920 K)[1] |
| Boiling point | 1530 °C (1800 K)[1] |
| Hazards: | Irritant |
| Structure | |
| Coordination geometry | octahedral (sic-coordinate)[3] |
| Crystal structure | AlCl3 structure[1] |
| Hydrates | hexahydrate |
| Related compounds | |
| dysprosium(II) chloride
dysprosium(III) fluoride dysprosium(III) bromide dysprosium(III) iodide | terbium(III) chloride
holmium(III) chloride californium(III) chloride |
Dysprosium(III) chloride (DyCl3), also known as dysprosium trichloride, is a compound of dysprosium and chlorine. It is a white to yellow solid which rapidly absorbs water on exposure to moist air to form a hexahydrate, DyCl3.6H2O. Simple rapid heating of the hydrate causes partial hydrolysis[1] to an oxychloride, DyOCl.
| Contents |
Chemical properties
Dysprosium(III) chloride is a moderately strong Lewis acid, which ranks as "hard" according to the Hard-Soft Acid-Base theory . Aqueous solutions of dysprosium chloride can be used to prepare insoluble dysprosium(III) compounds, for example dysprosium(III) fluoride :
DyCl3(aq) + 3 NaF(aq) → DyF3 (s) + 3 NaCl(aq)
Preparation
Dysprosium(III) chloride can be prepared as a yellow aqueous solution by reaction of either dysprosium metal or dysprosium(III) carbonate and hydrochloric acid. The anhydrous halide may alternatively be prepared from dysprosium metal and hydrogen chloride[6].
2 Dy(s) + 6 HCl(aq) → 2 DyCl3(aq) + 3 H2(g)
Dy2(CO3)3 (s) + 6 HCl(aq) → 2 DyCl3(aq) + 3 CO2(g) + 3 H2O(l)
Anhydrous DyCl3 can be made by dehydration of the hydrate either by slowly heating to 400 °C with 4-6 equivalents of ammonium chloride under high vacuum[1],[4]. The anhydrous halide may alternatively be prepared from dysprosium metal and hydrogen chloride[5]. It is usually purified by high temperature sublimation under high vacuum.[1]
Uses
Dysprosium(III) chloride can be used as a starting point for the preparation of other dysprosium salts.
Precautions
Dysprosium compounds are of low to moderate toxicity, although their toxicity has not been investigated in detail.
Suppliers/Manufacturers
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References
- F. T. Edelmann, P. Poremba, in: Synthetic Methods of Organometallic and Inorganic Chemistry, (W. A. Herrmann, ed.), Vol. 6, Georg Thieme Verlag, Stuttgart, 1997.
- CRC Handbook of Chemistry and Physics (58th edition), CRC Press, West Palm Beach, Florida, 1977.
- N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, Pergamon Press, 1984.
- M. D. Taylor, P. C. Carter, J. Inorg. Nucl. Chem. 24, 387 (1962); J. Kutscher, A. Schneider, Inorg. Nucl. Chem. Lett. 7, 815 (1971).
- L. F. Druding, J. D. Corbett, J. Am. Chem. Soc. 83, 2462 (1961); J. D. Corbett, Rev. Chim. Minerale 10, 239 (1973).
- G. A. Molander, E. D. Dowdy, in Lanthanides: Chemistry and Use in Organic Synthesis, Springer-Verlag, Berlin, 1999, p119-154.
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