Europium(III) chloride 1263271 224159445 2008-07-07T16:19:36Z VolkovBot 3035831 robot Modifying: [[zh:氯化铕(III)]] {{Chembox new | Name = Europium(III) chloride | ImageFile = Europium(III)_chloride_hexahydrate.jpg <!-- | ImageSize = 150px --> | ImageName = Crystals of europium(III) chloride hexahydrate | OtherNames = Europium trichloride | Section1 = {{Chembox Identifiers | CASOther = [10025-76-0] (''anhydr.'') | EINECS = 233-040-4 | RTECS = LE7525000 }} | Section2 = {{Chembox Properties | Formula = EuCl<sub>3</sub> | MolarMass = 258.32 g/mol (''anhydr.'') | Solvent = other solvents | SolubleOther = Soluble | MeltingPt = 632 °C ''decomp.''}} }} ''' Europium(III) chloride''' is a compound of [[europium]] and [[chlorine]] with the formula EuCl<sub>3</sub>. ==Properties== Europium trichloride is a yellow solid which begins to decompose at or below its melting point to give at least some [[europium(II) chloride|EuCl<sub>2</sub>]]. Being [[hygroscopic]] it rapidly absorbs water on exposure to moist air to form a white crystalline hexa[[hydrate]], EuCl<sub>3</sub>.6H<sub>2</sub>O (''M''<sub>r</sub>&nbsp;= 366.41 g/mol; [[CAS number]] [13759-92-7]). Simple rapid heating of the [[hydrate]] alone may cause small amounts of [[hydrolysis]]. [[Anhydrous]] EuCl<sub>3</sub> can be made from the hydrate by heating with an excess of [[thionyl chloride]] for around 15 hours.<ref>{{cite journal | author = Freeman, J.H. | coauthors = Smith, M.L. | year = 1958 | title = Preparation of Anhydrous Inorganic Chlorides by Dehydration with Thionyl Chloride | journal = [[J. Inorg. Nucl. Chem.]] | volume = 7 | pages = 224–227 | doi = 10.1016/0022-1902(58)80073-1}}</ref> Europium(III) chloride is soluble in [[water]]. When anhydrous, it is expected to be also highly [[soluble]] in [[ethanol]] (by analogy with [[samarium(III) chloride|SmCl<sub>3</sub>]]). It is nine-coordinate (trigonal prismatic), and it crystallises with the [[uranium(III) chloride|UCl<sub>3</sub>]] structure.<ref>{{Greenwood&Earnshaw}}</ref> ==Uses== Europium(III) chloride can be used for the preparation of [[europium(II) chloride]] by reduction in a gold boat using [[hydrogen]] gas while heating slowly to 700 °C. The anhydrous [[chloride]] may also be used to prepare [[organometallic]] compounds of europium, such as bis(pentamethylcyclopentadienyl)europium(II) complexes.<ref>{{cite journal | doi = 10.1021/ic50212a031 | year = 1980 | author = Tilley, T. Don | journal = Inorganic Chemistry | volume = 19 | pages = 2999 | title = Divalent lanthanide chemistry. Bis (pentamethylcyclopentadienyl) europium(II) and -ytterbium(II) derivatives: crystal structure of bis (pentamethylcyclopentadienyl) (tetrahydrofuran ytterbium(II) -hemitoluene at 176 K}}</ref><ref>{{cite journal | doi = 10.1021/om00138a001 | year = 1986 | author = Evans, William J. | journal = Organometallics | volume = 5 | pages = 1285 | title = Synthesis and x-ray crystal structure of bis(pentamethylcyclopentadienyl) complexes of samarium and europium: (C<sub>5</sub>Me<sub>5</sub>)<sub>2</sub>Sm and (C<sub>5</sub>Me<sub>5</sub>)<sub>2</sub>Eu}}</ref> Europium(III) chloride can be used as a starting point for the preparation of other [[europium]] [[salt]]s. ==Bibliography== * Edelmann, F. T.; & Poremba, P. (1997). in: ''Synthetic Methods of Organometallic and Inorganic Chemistry'' (Herrmann, E. A., Ed.) Vol. 6. Stuttgart:Georg Thieme. * {{RubberBible53rd}} ==References== <references/> [[Category:Chlorides]] [[Category:Europium compounds]] [[Category:Metal halides]] [[pl:Chlorek europu(III)]] [[zh:氯化铕(III)]]