|3D model (Jmol)||Interactive image|
|Molar mass||245.26 g/mol (anhydrous)
353.36 g/mol (hexahydrate)
371.37 g/mol (heptahydrate)
|Appearance||white odorless powder
|Melting point||858 °C (1,576 °F; 1,131 K) (anhydrous)|
|Boiling point||1,000 °C (1,830 °F; 1,270 K) (anhydrous)|
|Solubility||soluble in ethanol (heptahydrate)|
|hexagonal (UCl3 type), hP8|
|P63/m, No. 176|
|Tricapped trigonal prismatic,(nine-coordinate)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
The La3+ centre is 9-coordinate in the trichloride. The structure is similar to that for uranium trichloride.
Preparation and reactions
- 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.
Lanthanum chloride does not have many applications. A possible application involves the precipitation of phosphate from solutions, e.g. in swimming pools to prevent algae growth. 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.
This compound is also used in Gamma Detectors, is one of the smallest sized (massed) meters of the inorganic compounds used for Gamma Ray Detectors.
Lanthanum chloride is also frequently used as an ionisation suppressant in Atomic Emission spectroscopy.
- Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY.
- 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.
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