Scandium chloride

Scandium(III) chloride
IUPAC name

Scandium(III) chloride
Other names

scandium chloride
scandium trichloride
Identifiers
CAS number 10361-84-9
PubChem 82586
ChemSpider 74528 Y
RTECS number VQ8925000
Jmol-3D images Image 1
Properties
Molecular formula ScCl3
Molar mass 151.31 g/mol
Appearance grayish-white crystals
Density 2.39 g/mL, solid
Melting point

960 °C[1]
Solubility in water soluble
Solubility in other solvents insoluble in EtOH
Hazards
MSDS External MSDS
Main hazards irritant
Related compounds
Related compounds scandium(III) fluoride
scandium(III) nitrate
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Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

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] Scandium(III) chloride is mainly of interest in the research laboratory. Both the anhydrous form and hexahydrate (ScCl3•6H2O) are commercially available.

Contents

Chemical and physical properties

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 is bridged with four Sc-Cl bonds.[4]

Reactions

ScCl3 dissolves in water to give [Sc(H2O)]3+ ions. In fact, samples of ScCl3 converts to this hexahydrate upon exposure to air. 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.[5] 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.

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.[6]

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][7] For exampled, reduction of ScCl3 with scandium metal in the presence of caesium chloride gives the compound CsScCl3 which contain linear chains of composition ScCl3−.[2]

Uses

Scandium(III) chloride is found in some halide lamps, optical fibers, electronic ceramics, and lasers[8].

References

  1. ^ Frederikse, H.P.R.; Lide, David R. (1998). CRC Handbook of Chemistry and Physics (78th Edition)
  2. ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. ISBN 0080379419. 
  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. ^ a b 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. ^ Manzer, L. E., "Tetrahydrofuran Complexes of Selected Early Transition Metals", Inorganic Syntheses, 1982, volume 21, page 135-40.doi:10.1002/9780470132524.ch31
  6. ^ 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. 
  7. ^ Corbett, J.D. (1981). "Extended metal-metal bonding in halides of the early transition metals". Acc. Chem. Res. 14: 239–246. doi:10.1021/ar00068a003. 
  8. ^ Metal Suppliers Online. (2000). Scandium Chloride

External links