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| Names | |
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| IUPAC names
Dysprosium(III) chloride | |
| Identifiers | |
3D model (JSmol) |
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| ChemSpider |
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| ECHA InfoCard | 100.030.024 
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PubChem CID |
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| UNII | |
CompTox Dashboard (EPA) |
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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 labelling:[1] | |
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| Warning | |
| H315, H319, H335 | |
| P302+P352, P305+P351+P338 | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions |
Dysprosium(III) fluoride Dysprosium(III) bromide Dysprosium(III) iodide Dysprosium(III) oxide |
Other cations |
Terbium(III) chloride Dysprosium(II) chloride Holmium(III) chloride |
Related compounds |
Dysprosium(II) chloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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.
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]:
The pentachloride decomposes thermally according to the following equation:
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]
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:
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 DyCl3ineutectic LiCl-KCliselectrolysed. The reduction occurs via Dy2+, at a tungsten cathode.[6]
Dysprosium compounds are believed to be of low to moderate toxicity, although their toxicity has not been investigated in detail.
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