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Yttrium(III) chloride
	; Part of a layer in the crystal structure of YCl3
Unit cell	Layer packing
Names
	IUPAC names Yttrium(III) chloride; Yttrium trichloride
Identifiers
CAS Number	10361-92-9 ;
3D model (JSmol)	anhydrous: Interactive image; hexahydrate: Interactive image;
ChemSpider	59696 ; hexahydrate: 175148;
ECHA InfoCard	100.030.716
EC Number	hexahydrate: 233-801-0;
PubChem CID	10198055; hexahydrate: 16211498;
RTECS number	ZG3150000;
UNII	11521XLD38 ;
CompTox Dashboard (EPA)	DTXSID2042515 ;
	InChI InChI=1S/3ClH.Y/h31H;/q;;;+3/p-3 Key: PCMOZDDGXKIOLL-UHFFFAOYSA-K ; InChI=1/3ClH.Y/h31H;/q;;;+3/p-3 Key: PCMOZDDGXKIOLL-DFZHHIFOAW; hexahydrate: InChI=1S/3ClH.6H2O.Y/h31H;61H2;/q;;;;;;;;;+3/p-3 Key: IINACGXCEZNYTF-UHFFFAOYSA-K;
	SMILES anhydrous: [Y+3].[Cl-].[Cl-].[Cl-]; hexahydrate: [OH2+][Y-3]([OH2+])([OH2+])([OH2+])([OH2+])[OH2+].[Cl-].[Cl-].[Cl-];
Properties
Chemical formula	YCl3
Molar mass	195.265 g/mol
Appearance	white solid
Density	2.61 g/cm3
Melting point	721 °C (1,330 °F; 994 K)
Boiling point	1,482 °C (2,700 °F; 1,755 K)
Solubility in water	751 g/L (20 °C)
Solubility	601 g/L ethanol (15 °C); 606 g/L pyridine (15 °C)
Structure
Crystal structure	Monoclinic, mS16
Space group	C2/m, No. 12
Lattice constant	a = 0.692 nm, b = 1.194 nm, c = 0.644 nm α = 90°, β = 111°, γ = 90°
Formula units (Z)	4
Hazards
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H315, H319, H335
Precautionary statements	P261, P264, P271, P280, P302+P352, P304+P340, P305+P351+P338, P312, P332+P313, P337+P313, P362
NFPA 704 (fire diamond)	1 0 0
Safety data sheet (SDS)	External MSDS
Related compounds
Other anions	Yttrium(III) fluoride; Yttrium(III) bromide; Yttrium(III) iodide
Other cations	Scandium(III) chloride; Lutetium(III) chloride
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Yttrium(III) chloride is an inorganic compound of yttrium and chloride. It exists in two forms, the hydrate (YCl₃(H₂O)₆) and an anhydrous form (YCl₃). Both are colourless salts that are highly soluble in water and deliquescent.

Structure

Solid YCl₃ adopts a cubic^{[citation needed]} structure with close-packed chloride ions and yttrium ions filling one third of the octahedral holes and the resulting YCl₆ octahedra sharing three edges with adjacent octahedra, giving it a layered structure.^[5]^[1] This structure is shared by a range of compounds, notably AlCl₃.

Preparation and reactions

YCl₃ is often prepared by the "ammonium chloride route," starting from either Y₂O₃ or hydrated chloride or oxychloride.^[6]^[7] or YCl₃·6H₂O.^[8] These methods produce (NH₄)₂[YCl₅]:

10 NH₄Cl + Y₂O₃ → 2 (NH₄)₂[YCl₅] + 6 NH₃ + 3 H₂O

YCl₃·6H₂O + 2 NH₄Cl → (NH₄)₂[YCl₅] + 6 H₂O

The pentachloride decomposes thermally according to the following equation:

(NH₄)₂[YCl₅] → 2 NH₄Cl + YCl₃

The thermolysis reaction proceeds via the intermediacy of (NH₄)[Y₂Cl₇].

Treating Y₂O₃ with aqueous HCl produces the hydrated chloride (YCl₃·6H₂O). When heated, this salt yields yttrium oxychloride rather than reverting to the anhydrous form.

References

^ ^a ^b Templeton, D. H.; Carter, Giles F. (1954). "The Crystal Structures of Yttrium Trichloride and Similar Compounds". J. Phys. Chem. 58 (11): 940–944. doi:10.1021/j150521a002.
^ ^a ^b ^c ^d ^e Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.99. ISBN 978-1439855119.
^ Spencer, James F. (1919), The Metals of the Rare Earths, New York: Longmans, Green, and Co, p. 135
^ Templeton, D. H.; Carter, Giles F. (1954). "The Crystal Structures of Yttrium Trichloride and Similar Compounds". The Journal of Physical Chemistry. 58 (11): 940–944. doi:10.1021/j150521a002.
^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
^ 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.
^ Edelmann, F. T.; Poremba, P. (1997). Herrmann, W. A. (ed.). Synthetic Methods of Organometallic and Inorganic Chemistry. Vol. VI. Stuttgart: Georg Thieme Verlag. ISBN 978-3-13-103021-4.
^ 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.