Chemistry:Dysprosium(III) chloride
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| Names | |
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| IUPAC names
Dysprosium(III) chloride
Dysprosium trichloride | |
| Identifiers | |
3D model (JSmol)
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PubChem CID
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| Properties | |
| DyCl3 | |
| Molar mass | 268.86 g/mol (anhydrous) |
| Appearance | white solid |
| Density | 3.67 g/cm3, solid |
| Melting point | 647 °C (1,197 °F; 920 K) (anhydrous) |
| Boiling point | 1,530 °C (2,790 °F; 1,800 K) |
| Soluble | |
| Structure | |
| AlCl3 structure | |
| Octahedral | |
| Hazards | |
| GHS pictograms | 
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| GHS Signal word | warning |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
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Dysprosium(III) fluoride Dysprosium(III) bromide Dysprosium(III) iodide Dysprosium(III) oxide |
Other cations
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Terbium(III) chloride Dysprosium(II) chloride Holmium(III) chloride |
Related compounds
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Dysprosium(II) chloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
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[2] to an oxychloride, DyOCl.
Preparation and reactions
DyCl3 is often prepared by the "ammonium chloride route", starting from either Dy2O3 or the hydrated chloride DyCl3·6H2O.[3][4][5] These methods produce (NH4)2[DyCl5]:
- 10 NH4Cl + Dy2O3 → 2 (NH4)2[DyCl5] + 6 NH3 + 3 H2O
- DyCl3·6H2O + 2 NH4Cl → (NH4)2[DyCl5] + 6 H2O
The pentachloride decomposes thermally according to the following equation:
- (NH4)2[DyCl5] → 2 NH4Cl + DyCl3
The thermolysis reaction proceeds via the intermediacy of (NH4)[Dy2Cl7].
Treating Dy2O3 with aqueous HCl produces the hydrated chloride DyCl3·6H2O, which cannot be rendered anhydrous by heating. Instead one obtains an oxychloride:[4]
- DyCl3 + H2O → DyOCl + 2 HCl
Dysprosium(III) chloride is a moderately strong Lewis acid, which ranks as "hard" according to the HSAB concept. Aqueous solutions of dysprosium chloride can be used to prepare other dysprosium(III) compounds, for example dysprosium(III) fluoride:
- DyCl3 + 3 NaF → DyF3 + 3 NaCl
Uses
Dysprosium(III) chloride can be used as a starting point for the preparation of other dysprosium salts. Dysprosium metal is produced when a molten mixture of DyCl3 in eutectic LiCl-KCl is electrolysed. The reduction occurs via Dy2+, at a tungsten cathode.[6]
Precautions
Dysprosium compounds are believed to be of low to moderate toxicity, although their toxicity has not been investigated in detail.
References
- ↑ GHS: Sigma-Aldrich 325546
- ↑ F. T. Edelmann, P. Poremba, in: Synthetic Methods of Organometallic and Inorganic Chemistry, (W. A. Herrmann, ed.), Vol. 6, Georg Thieme Verlag, Stuttgart, 1997.
- ↑ Meyer, G. (1989). "The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides—The Example of Ycl 3". The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides-The Example of YCl3. Inorganic Syntheses. 25. pp. 146–150. doi:10.1002/9780470132562.ch35. ISBN 978-0-470-13256-2.
- ↑ 4.0 4.1 Taylor, M.D.; Carter, C.P. (1962). "Preparation of anhydrous lanthanide halides, especially iodides". Journal of Inorganic and Nuclear Chemistry 24 (4): 387–391. doi:10.1016/0022-1902(62)80034-7.
- ↑ Edelmann, F. T.; Poremba, P. (1997). Herrmann, W. A.. ed. Synthetic Methods of Organometallic and Inorganic Chemistry. VI. Stuttgart: Georg Thieme Verlag. ISBN 3-13-103021-6.
- ↑ Y. Castrillejo, M. R. Bermejo, A. I. Barrado, R. Pardo, E. Barrado, A. M. Martinez, Electrochimica Acta, 50, 2047-2057 (2005).
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