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Dysprosium(III) chloride

Names
IUPAC names Dysprosium(III) chloride Dysprosium trichloride
Identifiers
CAS Number	10025-74-8
3D model (JSmol)	Interactive image
ChemSpider	59592
ECHA InfoCard	100.030.024
PubChem CID	66207
UNII	Q2A03W637H
CompTox Dashboard (EPA)	DTXSID8041909
InChI InChI=1S/3ClH.Dy/h3*1H;/q;;;+3/p-3Key: BOXVSFHSLKQLNZ-UHFFFAOYSA-K InChI=1/3ClH.Dy/h3*1H;/q;;;+3/p-3Key: BOXVSFHSLKQLNZ-DFZHHIFOAK
SMILES Cl(Cl)Cl
Properties
Chemical formula	DyCl3
Molar mass	268.86 g/mol (anhydrous)
Appearance	white solid
Density	3.67 g/cm, solid
Melting point	647 °C (1,197 °F; 920 K) (anhydrous)
Boiling point	1,530 °C (2,790 °F; 1,800 K)
Solubility in water	Soluble
Structure
Crystal structure	AlCl3 structure
Coordination geometry	Octahedral
Hazards
GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H315, H319, H335
Precautionary statements	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 , 100 kPa). N verify (what is  ?) 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 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. These methods produce (NH₄)₂:

10 NH₄Cl + Dy₂O₃ → 2 (NH₄)₂ + 6 NH₃ + 3 H₂O

DyCl₃·6H₂O + 2 NH₄Cl → (NH₄)₂ + 6 H₂O

The pentachloride decomposes thermally according to the following equation:

(NH₄)₂ → 2 NH₄Cl + DyCl₃

The thermolysis reaction proceeds via the intermediacy of (NH₄).

Treating Dy₂O₃ with aqueous HCl produces the hydrated chloride DyCl₃·6H₂O, which cannot be rendered anhydrous by heating. Instead one obtains an oxychloride:

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 Dy, at a tungsten cathode.

Precautions

Dysprosium compounds are believed to be of low to moderate toxicity, although their toxicity has not been investigated in detail.

References

1. GHS: Sigma-Aldrich 325546
2. F. T. Edelmann, P. Poremba, in: Synthetic Methods of Organometallic and Inorganic Chemistry, (W. A. Herrmann, ed.), Vol. 6, Georg Thieme Verlag, Stuttgart, 1997.
3. 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. Vol. 25. pp. 146–150. doi:10.1002/9780470132562.ch35. ISBN 978-0-470-13256-2.
4. ^ 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.
5. Edelmann, F. T.; Poremba, P. (1997). Herrmann, W. A. (ed.). Synthetic Methods of Organometallic and Inorganic Chemistry. Vol. VI. Stuttgart: Georg Thieme Verlag. ISBN 3-13-103021-6.
6. Y. Castrillejo, M. R. Bermejo, A. I. Barrado, R. Pardo, E. Barrado, A. M. Martinez, Electrochimica Acta, 50, 2047-2057 (2005).

• Dysprosium compounds
• Chlorides
• Lanthanide halides