Scandium chloride

Scandium(III) chloride is the inorganic compound with the formula ScCl3. It is a white, high-melting ionic compound, which is deliquescent and highly water-soluble.[2] This salt is mainly of interest in the research laboratory. Both the anhydrous form and hexahydrate (ScCl3•6H2O) are commercially available.

Scandium(III) chloride
Names
IUPAC name
Scandium(III) chloride
Other names
scandium chloride
scandium trichloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.714
RTECS number
  • VQ8925000
UNII
  • InChI=1S/3ClH.Sc/h3*1H;/q;;;+3/p-3 checkY
    Key: DVMZCYSFPFUKKE-UHFFFAOYSA-K checkY
  • InChI=1/3ClH.Sc/h3*1H;/q;;;+3/p-3
    Key: DVMZCYSFPFUKKE-DFZHHIFOAN
  • InChI=1S/3ClH.Sc/h3*1H;/q;;;+3/p-3
    Key: DVMZCYSFPFUKKE-UHFFFAOYSA-K
  • Cl[Sc](Cl)Cl
Properties
ScCl3
Molar mass 151.31 g/mol
Appearance grayish-white crystals
Density 2.39 g/mL, 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 in EtOH
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 irritant
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond
1
0
Lethal dose or concentration (LD, LC):
3980 mg/kg (mouse, oral)
Safety data sheet (SDS) External MSDS
Related compounds
Other anions
 Scandium(III) fluoride
Scandium bromide
Scandium triiodide
Other cations
 Yttrium(III) chloride
Lutetium(III) chloride
Related compounds
 Scandium(III) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)
Infobox references

Structure

ScCl3 crystallises in the layered BiI3 motif, which features octahedral scandium centres.[3] Monomeric ScCl3 is the predominant species in the vapour phase at 900 K, the dimer Sc2Cl6 accounts for approximately 8%.[4] The electron diffraction spectrum indicates that the monomer is planar and the dimer has two bridging Cl atoms each Sc being 4 coordinate.[4]

Reactions
Structure of trans-[Sc(H2O)4Cl2]+.

ScCl3 is a Lewis acid that absorbs water to give aquo complexes. According to X-ray crystallogrphy, one such hydrate is the salt trans-[ScCl2(H2O)4]Cl·2H2O.[5] With the less basic ligand tetrahydrofuran, ScCl3 yields the adduct ScCl3(THF)3 as white crystals. This THF-soluble complex is used in the synthesis of organoscandium compounds.[6] ScCl3 has been converted to its dodecyl sulfate salt, which has been investigated as a "Lewis acid-surfactant combined catalyst" (LASC) in aldol-like reactions.[7]

Reduction

Scandium(III) chloride was used by Fischer et al. who first prepared metallic scandium by electrolysis of a eutectic melt of scandium(III) chloride and other salts at 700-800 °C.[8]

ScCl3 reacts with scandium metal to give a number of chlorides where scandium has an oxidation state <+3, ScCl, Sc7Cl10, Sc2Cl3, Sc5Cl8 and Sc7Cl12.[2][9] For example, reduction of ScCl3 with scandium metal in the presence of caesium chloride gives the compound CsScCl3 which contain linear chains of composition ScIICl3−, containing ScIICl6 octahedra sharing faces.[10]

Uses

Scandium(III) chloride is found in some halide lamps, optical fibers, electronic ceramics, and lasers.[11]

References
  1. Frederikse, H.P.R.; Lide, David R. (1998). CRC Handbook of Chemistry and Physics (78th Edition)
  2. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  3. Crystal Structure of ScCl3 Refined from Powder Neutron Diffraction Data, Fjellvåg, H., Karen, P., Acta Chemica Scandinavica, 48, 294-297, doi:10.3891/acta.chem.scand.48-0294
  4. Haaland A., Martinsen K-G, Shorokhov D.J, Girichev G.V., Sokolov V.I, J. Chem. Soc., Dalton Trans., 1998, 2787 - 2792, doi:10.1039/a803339k
  5. The Rare Earth Elements, Fundamentals and Applications David A. Atwood, 2012, John Wiley & Sons Inc, ISBN 9781119950974
  6. Manzer, L. E., "Tetrahydrofuran Complexes of Selected Early Transition Metals", Inorganic Syntheses, 1982, volume 21, page 135-40.doi:10.1002/9780470132524.ch31
  7. Manabe, Kei; Mori, Yuichiro; Kobayashi, Shū (1999). "Effects of Lewis acid-surfactant-combined catalysts on aldol and Diels-Alder reactions in water". Tetrahedron. 55 (37): 11203–11208. doi:10.1016/S0040-4020(99)00642-0.
  8. Fischer, Werner; Brünger, Karl; Grieneisen, Hans (1937). "Über das metallische Scandium". Zeitschrift für anorganische und allgemeine Chemie. 231 (1–2): 54–62. doi:10.1002/zaac.19372310107.
  9. Corbett, J.D. (1981). "Extended metal-metal bonding in halides of the early transition metals". Acc. Chem. Res. 14 (8): 239–246. doi:10.1021/ar00068a003.
  10. Meyer, Gerd.; Corbett, John D. (1981). "Reduced ternary halides of scandium: RbScX3 (X = chlorine, bromine) and CsScX3 (X = chlorine, bromine, iodine)". Inorganic Chemistry. 20 (8): 2627–2631. doi:10.1021/ic50222a047. ISSN 0020-1669.
  11. Metal Suppliers Online. (2000). Scandium Chloride


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