Dysprosium(III) chloride
_chloride.jpg)
| |
| Names | |
|---|---|
| IUPAC names
Dysprosium(III) chloride
Dysprosium trichloride | |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.030.024 |
PubChem CID
|
|
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| DyCl3 | |
| Molar mass | 268.86 g/mol (anhydrous) |
| Appearance | white solid |
| Density | 3.67 g/cm³, solid |
| Melting point | 647 °C (anhydrous) |
| Boiling point | 1530 °C |
| Soluble | |
| Structure | |
| AlCl3 structure | |
| Octahedral | |
| Hazards | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
|
Dysprosium(III) fluoride Dysprosium(III) bromide Dysprosium(III) iodide |
Other cations
|
Terbium(III) chloride Dysprosium(II) chloride Holmium(III) 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[1] to an oxychloride, DyOCl.
Preparation and reactions
DyCl3 is often prepared by the "ammonium chloride route," starting from either Dy2O3 or hydrated chloride or oxychloride.[2][3] or DyCl3·6H2O.[4] 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 hydrated chloride (DyCl3·6H2O). This salt cannot be rendered anhydrous by heating. Instead one obtains an oxychloride.
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.[5]
Precautions
Dysprosium compounds are believed to be of low to moderate toxicity, although their toxicity has not been investigated in detail.
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.
- ^ Meyer, G. (1989). "The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides-The Example of YCl3". Inorganic Syntheses. 25: 146–150. doi:10.1002/9780470132562.ch35. ISBN 978-0-470-13256-2.
- ^ Edelmann, F. T. (1997). Herrmann, W. A. (ed.) (ed.). Synthetic Methods of Organometallic and Inorganic Chemistry. Vol. VI. Stuttgart: Georg Thieme Verlag. ISBN 3-13-103021-6.
{{cite book}}:|editor=has generic name (help); Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Taylor, M.D. "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.
{{cite journal}}: Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Y. Castrillejo, M. R. Bermejo, A. I. Barrado, R. Pardo, E. Barrado, A. M. Martinez, Electrochimica Acta, 50, 2047-2057 (2005).