Dysprosium(III) chloride

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/h31H;/q;;;+3/p-3 Key: BOXVSFHSLKQLNZ-UHFFFAOYSA-K ; InChI=1/3ClH.Dy/h31H;/q;;;+3/p-3 Key: BOXVSFHSLKQLNZ-DFZHHIFOAK;
	SMILES Cl[Dy](Cl)Cl;
Properties
Chemical formula	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)
Solubility in water	Soluble
Structure
Crystal structure	AlCl3 structure
Coordination geometry	Octahedral
Hazards
EU classification (DSD) (outdated)	not listed
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).
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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[1] 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.[2][3][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 the hydrated chloride DyCl₃·6H₂O, which cannot be rendered anhydrous by heating. Instead one obtains an oxychloride:[3]

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.[5]

Precautions

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

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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. pp. 146–150. doi:10.1002/9780470132562.ch35. ISBN 978-0-470-13256-2.
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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[Edel-1] F. T. Edelmann, P. Poremba, in: Synthetic Methods of Organometallic and Inorganic Chemistry, (W. A. Herrmann, ed.), Vol. 6, Georg Thieme Verlag, Stuttgart, 1997.

[2] Meyer, G. (1989). 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.

[Taylor-3] 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.

[EdelmannPoremba1997-4] 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.

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