 Crystals of scandium(III) chloride hexahydrate | |
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| Names | |
|---|---|
| IUPAC name Scandium(III) chloride | |
Other names
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| Identifiers | |
3D model (JSmol) | |
| ChemSpider |
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| ECHA InfoCard | 100.030.714 |
| RTECS number |
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| UNII | |
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| Properties | |
| ScCl3 | |
| Molar mass | 151.31 g·mol−1 |
| Appearance | grayish-white crystals |
| Density | 2.39 g/cm3, solid |
| Melting point | 960 °C (1,760 °F; 1,230 K)[1] 63 °C (hexahydrate) |
| 70.2 g/100 mL | |
| Solubility in other solvents | soluble in alcohol,acetone,glycerin insoluble inEtOH[citation needed] |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | irritant |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) | 3980 mg/kg (mouse, oral) |
| Safety data sheet (SDS) | External MSDS |
| Related compounds | |
Otheranions | |
Othercations | |
Related compounds | Scandium(III) nitrate |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Scandium(III) chloride is aninorganic compound with theformulaScCl3. It is a white, high-meltingionic compound, which isdeliquescent and highly water-soluble.[2] This salt is mainly of interest in the research laboratory. Both theanhydrous form andhexahydrate (ScCl3·6H2O) are commercially available.
ScCl3 crystallises in the layeredBiI3 motif, which featuresoctahedral scandium centres.[3] MonomericScCl3 is the predominant species in thevapour phase at 900 K, thedimerSc2Cl6 accounts for approximately 8%.[4] Theelectron diffraction spectrum indicates that themonomer is planar and the dimer has two bridging Cl atoms each Sc being4 coordinate.[4]
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ScCl3 is aLewis acid that absorbs water to giveaquo complexes. According toX-ray crystallogrphy, one such hydrate is the salttrans-[ScCl2(H2O)4]Cl·2H2O.[5] With the less basicligandtetrahydrofuran,ScCl3 yields theadductScCl3(THF)3 as white crystals. ThisTHF-solublecomplex is used in the synthesis oforganoscandium compounds.[6]ScCl3 has been converted to its dodecyl sulfate salt, which has been investigated as a "Lewis acid-surfactant combined catalyst" (LASC) inaldol-like reactions.[7]
Scandium(III) chloride was used by Fischer et al. who first prepared metallic scandium byelectrolysis of aeutectic melt of scandium(III) chloride and other salts at 700-800 °C.[8]
ScCl3 reacts with scandium metal to give a number ofchlorides where scandium has anoxidation state of less than +3, ScCl,Sc7Cl10,Sc2Cl3,Sc5Cl8 andSc7Cl12.[2][9] For example,reduction ofScCl3 with scandium metal in the presence ofcaesium chloride gives the compoundCsScCl3 which contain linear chains of compositionScIICl−3, containingScIICl6 octahedra sharing faces.[10]
Scandium(III) chloride is found in somehalide lamps,optical fibers,electronic ceramics, andlasers.[11]
