| 词条 | Samarium(III) chloride |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 464386772 | ImageFile1 = Samarium(III) chloride hexahydrate.jpg | ImageName1 = Samarium(III)_chloride_hexahydrate | ImageFile2 = UCl3 without caption.png | IUPACName = Samarium(III) chloride | OtherNames = |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 55428 | InChI = 1/3ClH.Sm/h3*1H;/q;;;+3/p-3 | InChIKey = BHXBZLPMVFUQBQ-DFZHHIFOAZ | SMILES = Cl[Sm](Cl)Cl | UNII_Ref = {{fdacite|changed|FDA}} | UNII = 5J4QGH7J16 | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/3ClH.Sm/h3*1H;/q;;;+3/p-3 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = BHXBZLPMVFUQBQ-UHFFFAOYSA-K | CASNo = 10361-82-7 | CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Comment = (anhydrous) | CASNo1_Ref = {{cascite|correct|??}} | CASNo1 = 13465-55-9 | CASNo1_Comment = (hexahydrate) | PubChem = }} |Section2={{Chembox Properties | Formula = SmCl3 | MolarMass = 256.76 g/mol (anhydrous) 364.80 g/mol (hexahydrate) | Appearance = pale yellow solid (anhydrous) cream-coloured solid (hexahydrate) | Density = 4.46 g/cm3 (anhydrous) 2.383 g/cm3 (hexahydrate) | MeltingPtC = 682 | BoilingPt = decomposes | Solubility = 92.4 g/100 mL (10 °C) }} |Section3={{Chembox Structure | CrystalStruct = hexagonal, hP8 | SpaceGroup = P63/m, No. 176 | Coordination = Tricapped trigonal prismatic (nine-coordinate) |Section7={{Chembox Hazards | MainHazards = Irritant | FlashPt = | AutoignitionPt = }} |Section8={{Chembox Related | OtherAnions = Samarium(III) oxide | OtherCations = Promethium(III) chloride, Europium(III) chloride }} Samarium(III) chloride, also known as samarium trichloride, is an inorganic compound of samarium and chloride. It is a pale yellow solid that rapidly absorbs water to form a hexahydrate, SmCl3.6H2O.[1] The compound has few practical applications but is used in laboratories for research on new compounds of samarium. StructureLike several related chlorides of the lanthanides and actinides, SmCl3 crystallises in the UCl3 motif. The Sm3+ centres are nine-coordinate, occupying trigonal prismatic sites with additional chloride ligands occupying the three square faces. Preparation and reactionsSmCl3 is prepared by the "ammonium chloride" route, which involves the initial synthesis of (NH4)2[SmCl5]. This material can be prepared from the common starting materials at reaction temperatures of 230 °C from samarium oxide:[2] 10 NH4Cl + Sm2O3 → 2 (NH4)2[SmCl5] + 6 NH3 + 3 H2O The pentachloride is then heated to 350-400 °C resulting in evolution of ammonium chloride and leaving a residue of the anhydrous trichloride: (NH4)2[SmCl5] → 2 NH4Cl + SmCl3 It can also be prepared from samarium metal and hydrogen chloride.[3][4] 2 Sm + 6 HCl → 2 SmCl3 + 3 H2 Aqueous solutions of samarium(III) chloride can be prepared by dissolving metallic samarium or samarium carbonate in hydrochloric acid. Samarium(III) chloride is a moderately strong Lewis acid, which ranks as "hard" according to the HSAB concept. Aqueous solutions of samarium chloride can be used to prepare samarium trifluoride: SmCl3 + 3 KF → SmF3 + 3 KCl UsesSamarium(III) chloride is used for the preparation of samarium metal, which has a variety of uses, notably in magnets. Anhydrous SmCl3 is mixed with sodium chloride or calcium chloride to give a low melting point eutectic mixture. Electrolysis of this molten salt solution gives the free metal.[5] In laboratorySamarium(III) chloride can also be used as a starting point for the preparation of other samarium salts. The anhydrous chloride is used to prepare organometallic compounds of samarium, such as bis(pentamethylcyclopentadienyl)alkylsamarium(III) complexes.[6] References1. ^{{cite book | author = F. T. Edelmann, P. Poremba | title = Synthetic Methods of Organometallic and Inorganic Chemistry | editor = W. A. Herrmann | volume = 6 | publisher = Georg Thieme Verlag | location = Stuttgart | year = 1997}} {{Samarium compounds}}2. ^{{cite journal| last =Meyer| first =G.| title =The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides-The Example of YCl3| journal =Inorganic Syntheses| volume =25| year =1989| pages =146–150| doi =10.1002/9780470132562.ch35| isbn =978-0-470-13256-2}} 3. ^{{cite journal | doi = 10.1021/ja01472a010 | author = L. F. Druding, J. D. Corbett | journal = J. Am. Chem. Soc. | volume = 83 | pages = 2462 | year = 1961 | issue = 11}} 4. ^{{cite journal | author = J. D. Corbett | journal = Rev. Chim. Minerale | volume = 10 | pages = 239 | year = 1973}} 5. ^{{Greenwood&Earnshaw1st}} 6. ^{{cite book | author = G. A. Molander, E. D. Dowdy | editor = Shu Kobayashi | title = Lanthanides: Chemistry and Use in Organic Synthesis| publisher = Springer-Verlag | location = Berlin | year = 1999 | pages = 119–154 | isbn = 3-540-64526-8}} 3 : Chlorides|Samarium compounds|Metal halides |
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