Yttrium(III) chloride

Yttrium(III) chloride
Names
	IUPAC names Yttrium(III) chloride; Yttrium trichloride
Identifiers
CAS Number	10361-92-9 ;
3D model (JSmol)	Interactive image;
ChemSpider	59696 ;
ECHA InfoCard	100.030.716
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;
	SMILES Cl[Y](Cl)Cl;
Properties
Chemical formula	YCl3
Molar mass	195.265 g/mol[1]
Appearance	white solid
Density	2.61 g/cm3[1]
Melting point	721 °C (1,330 °F; 994 K)[1]
Boiling point	1,482 °C (2,700 °F; 1,755 K)[1]
Solubility in water	751 g/L (20 °C)[1]
Solubility	601 g/L ethanol (15 °C); 606 g/L pyridine (15 °C)[2]
Structure[3]
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 pictograms
GHS Signal word	Danger
Flash point	Non-flammable
Related compounds
Other anions	Yttrium(III) fluoride; Yttrium(III) bromide; Yttrium(III) iodide
Other cations	Scandium(III) chloride; Lanthanum(III) chloride; Actinium(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 solids that are highly soluble in water and deliquescent.

Structure

Solid YCl₃ adopts a cubic 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.[4] 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.[5][6] or YCl₃·6H₂O.[7] 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

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 YCl₃. Inorganic Syntheses. 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. 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.

This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.

[crc-1] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.99. ISBN 978-1439855119.

[rare-2] Spencer, James F. (1919), The Metals of the Rare Earths, New York: Longmans, Green, and Co, p. 135

[3] 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.

[4] Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6

[5] 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.

[EdelmannPoremba1997-6] Edelmann, F. T.; Poremba, P. (1997). Herrmann, W. A. (ed.). Synthetic Methods of Organometallic and Inorganic Chemistry. VI. Stuttgart: Georg Thieme Verlag. ISBN 978-3-13-103021-4.

[7] 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.