Dysprosium(III) chloride

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Dysprosium(III) chloride

General
Systematic name	Dysprosium(III) chloride Dysprosium trichloride
Molecular formula	DyCl₃
Molar mass	268.86 g/mol (anhydrous)
Appearance	white solid
CAS number	[10025-74-8]
Properties
Density and phase	3.67 g/cm³, solid
Solubility in water	Soluble
Melting point	647 °C (anhydrous)
Boiling point	1530 °C
Structure
Coordination geometry	Octahedral
Crystal structure	AlCl₃ structure
Hazards
MSDS	External MSDS
EU classification	not listed
NFPA 704
Flash point	non flammable
RTECS number	?
Supplementary data page
Structure and properties	n, ε_r, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
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 noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and 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^[1] to an oxychloride, DyOCl.

1 Chemical properties
2 Preparation
3 Uses
4 Precautions
5 References
6 External links

[edit] Chemical properties

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 insoluble dysprosium(III) compounds, for example dysprosium(III) fluoride:

DyCl₃(aq) + 3 NaF(aq) → DyF₃(s) + 3 NaCl(aq)

[edit] 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.

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]

[edit] 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.^[7]

[edit] Precautions

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

[edit] 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.
Y. Castrillejo, M. R. Bermejo, A. I. Barrado, R. Pardo, E. Barrado, A. M. Martinez, Electrochimica Acta, 50, 2047-2057 (2005).