Lanthanum(III) chloride

Lanthanum(III) chloride
Names
	Other names Lanthanum trichloride
Identifiers
CAS Number	10099-58-8 ; 10025-84-0 (heptahydrate) ;
3D model (JSmol)	Interactive image;
ChemSpider	58275 ;
ECHA InfoCard	100.030.202
EC Number	233-237-5;
PubChem CID	64735;
UNII	04M8624OXV ; 936G1MX96X (heptahydrate) ;
CompTox Dashboard (EPA)	DTXSID2051502 ;
	InChI InChI=1S/3ClH.La/h31H;/q;;;+3/p-3 Key: ICAKDTKJOYSXGC-UHFFFAOYSA-K ; InChI=1/3ClH.La/h31H;/q;;;+3/p-3 Key: ICAKDTKJOYSXGC-DFZHHIFOAJ;
	SMILES Cl[La](Cl)Cl;
Properties
Chemical formula	LaCl3
Molar mass	245.264 g/mol (anhydrous) ; 353.36 g/mol (hexahydrate) ; 371.37 g/mol (heptahydrate)
Appearance	white odorless powder ; hygroscopic
Density	3.84 g/cm3[1]
Melting point	858 °C (1,576 °F; 1,131 K) (anhydrous)[1]
Boiling point	1,000 °C (1,830 °F; 1,270 K) (anhydrous)
Solubility in water	957 g/L (25 °C)[1]
Solubility	soluble in ethanol (heptahydrate)
Structure[2]
Crystal structure	hexagonal (UCl3 type), hP8
Space group	P63/m, No. 176
Lattice constant	a = 0.74779 nm, b = 0.74779 nm, c = 0.43745 nm
Formula units (Z)	2
Coordination geometry	Tricapped trigonal prismatic,(nine-coordinate)
Related compounds
Other anions	Lanthanum oxide
Other cations	Cerium(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

Lanthanum chloride is the inorganic compound with the formula La Cl₃. It is a common salt of lanthanum which is mainly used in research. It is a white solid that is highly soluble in water and alcohols.

Preparation and reactions

It forms upon union of the elements, but a more commonly used method involves heating a mixture of lanthanum(III) oxide and ammonium chloride at 200–250 °C:[3]

La₂O₃ + 6 NH₄Cl → 2 LaCl₃ + 6 NH₃ + 2 H₂O

From the trichloride, one can produce the other trihalides by exchange. Reduction with potassium gives metallic lanthanum.

Uses

One application of lanthanum chloride is the removal of phosphate from solutions via precipitation, e.g. in swimming pools to prevent algae growth and other wastewater treatments.[4][5] It has also shown use as a filter aid and an effective flocculent. Lanthanum chloride is also used in biochemical research to block the activity of divalent cation channels, mainly calcium channels. Doped with cerium, it is used as a scintillator material.[6]

In organic synthesis, lanthanum trichloride functions as a mild Lewis acid for converting aldehydes to acetals.[7]

The compound has been identified as a catalyst for the high pressure oxidative chlorination of methane to chloromethane with hydrochloric acid and oxygen.[8]

References

Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.69. ISBN 978-1439855119.
Morosin, B (1968). "Crystal Structures of Anhydrous Rare‐Earth Chlorides". The Journal of Chemical Physics. 49 (7): 3007–3012. doi:10.1063/1.1670543.
Brauer, G., ed. (1963). Handbook of Preparative Inorganic Chemistry (2nd ed.). New York: Academic Press.
Ghassemi, Masood; Recht, Howard Leonard (1971). Phosphate Precipitation with Ferrous Iron.
"Water Treatment Chemicals". American Elements. Retrieved 2018-08-03.
Martin, T; Allier, C; Bernard, F (2007). "Lanthanum Chloride Scintillator for X-ray Detection". AIP Conference Proceedings. 879. pp. 1156–1159. doi:10.1063/1.2436269.
"Lanthanum trichloride: An efficient Lewis acid catalyst for chemo and regioselective enamination of β-dicarbonyl compounds". Arkivoc. 2007 (13): 204. 2007. doi:10.3998/ark.5550190.0008.d23.
Podkolzin SG, Stangland EE, Jones ME, Peringer E, Lercher JA (2007). "Methyl chloride production from methane over lanthanum-based catalysts". J. Am. Chem. Soc. 129 (9): 2569–76. doi:10.1021/ja066913w. PMID 17295483.

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

[r1-1] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.69. ISBN 978-1439855119.

[2] Morosin, B (1968). "Crystal Structures of Anhydrous Rare‐Earth Chlorides". The Journal of Chemical Physics. 49 (7): 3007–3012. doi:10.1063/1.1670543.

[Brauer-3] Brauer, G., ed. (1963). Handbook of Preparative Inorganic Chemistry (2nd ed.). New York: Academic Press.

[4] Ghassemi, Masood; Recht, Howard Leonard (1971). Phosphate Precipitation with Ferrous Iron.

[5] "Water Treatment Chemicals". American Elements. Retrieved 2018-08-03.

[6] Martin, T; Allier, C; Bernard, F (2007). "Lanthanum Chloride Scintillator for X-ray Detection". AIP Conference Proceedings. 879. pp. 1156–1159. doi:10.1063/1.2436269.

[7] "Lanthanum trichloride: An efficient Lewis acid catalyst for chemo and regioselective enamination of β-dicarbonyl compounds". Arkivoc. 2007 (13): 204. 2007. doi:10.3998/ark.5550190.0008.d23.

[pmid17295483-8] Podkolzin SG, Stangland EE, Jones ME, Peringer E, Lercher JA (2007). "Methyl chloride production from methane over lanthanum-based catalysts". J. Am. Chem. Soc. 129 (9): 2569–76. doi:10.1021/ja066913w. PMID 17295483.