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Scandium(III) chloride



Scandium(III) chloride
General
Other names scandium chloride
scandium trichloride
Molecular formula ScCl3
Molar mass 151.31 g/mol
Appearance grayish-white crystals
CAS number [10361-84-9]
Properties
Density and phase 2.39 g/mL, solid
Solubility soluble in H2O
insoluble in EtOH
Stability strongly hygroscopic
Melting point 960 °C
Boiling point  ?°C
Std enthalpy change
of fusion
, ΔfusHo
-925.1 kJ/mol
Crystal Structure hexagonal close-packed
Hazards
MSDS External MSDS
Main hazards irritant
NFPA 704
0
1
0
 
RTECS number VQ8925000
Related compounds
Related compounds scandium(III) fluoride
scandium(III) nitrate
Except where noted otherwise, data are given for
materials in their standard state (at 25 °C, 100 kPa)
Infobox disclaimer and references

Scandium(III) chloride is an ionic compound also known as scandium chloride and scandium trichloride. It is composed of one scandium and three chlorine atoms. Each chlorine atom takes one of scandium’s three valence electrons, resulting in 3Cl- and Sc3+. The ensuing formula is ScCl3[1].

Additional recommended knowledge

Contents

Chemical and physical properties

Scandium(III) chloride is a white crystalline solid with the formula ScCl3. Typical for an ionic solid, it is high-melting, liquefying at 960 °C[2]. Both exhibit hexagonal close-packed (hcp) crystal structures, but it is their bond energy that accounts for the melting points’ difference. Scandium(III) chloride is primarily of interest in the research laboratory and numerous suppliers (see below) offer both the anhydrous form and hexahydrate (ScCl3•6H2O).

Like other compounds of Sc, the chlorides are dominated by the III oxidation state. Interesting reduced forms of Sc can however be prepared by reducing the trichloride with Sc metal (see below).

Preparation[3]

Scandium(III) chloride is synthesized by the action of hydrogen chloride on elemental scandium or scandium(III) oxide. Carbon tetrachloride can also be used:

2Sc(s) + 6HCl(l) → 2ScCl3(s) + 3H2(g)

Reactions of scandium(III) chloride

  • Scandium(III) chloride’s was used in the first preparation of metallic scandium in 1937. Fischer and collaborators synthesized the metal through an electrolysis of a eutectic melt of scandium(III) chloride and other salts at 700-800 °C.[4].
  • Reaction of ScCl3 with tetrahydrofuran yields ScCl3(THF)3 as white crystals. This THF-soluble complex is a key synthetic intermediate.
  • ScCl3 has been converted to its dodecyl sulfate salt, which is used as a "Lewis acid-surfactant combined catalyst" (LASC) in aldol-like reactions.
  • ScCl3 has proven to be reactive toward Sc metal to give rise to a broad family of scandium chlorides where the Sc has an oxidation state <3.
Sc(s) + ScCl3 (950 °C) → Sc5Cl8
Sc(s) + ScCl3 (890 °C) → Sc7Cl12 → Sc(Sc6Cl12)

Other uses

Scandium(III) chloride is found in halide lamps, optical fibers, electronic ceramics, and lasers[5].

Handling and safety considerations

Scandium(III) chloride is hygroscopic it should be stored in a desiccator.

References

  1. ^ Greenwood, N.N.; Earnshaw, A. (1998). Chemistry of the Elements (2nd Edition).
  2. ^ Frederikse, H.P.R.; Lide, David R. (1998). CRC Handbook of Chemistry and Physics (78th Edition).
  3. ^ Subbarao, E.C.; Wallace, W.E. (1980) Science and Technology of Rare Earth Metals. (Academic Press) pp. 16
  4. ^ Metal Suppliers Online. (2000). Scandium Chloride.
  5. ^ Metall Rare Earth Limited. (2006). Scandium Chloride

Journal citations

  • Manzer, L. E., "Tetrahydrofuran Complexes of Selected Early Transition Metals", Inorganic Syntheses, 1982, volume 21, page 135-40.
  • Hwu, S. J.; Dudis, D. S. and Corbett, J. D., "Synthesis, structure, and properties of the infinite-chain compounds scandium chloride carbide, Sc5Cl8C and scandium chloride nitride, Sc5Cl8N", Inorganic Chemistry, 1987, volume 26, page 469-73
  • Corbett, J. D., "Trichlorides of the rare earth elements, yttrium, and scandium", Inorganic Syntheses, 1983, volume 22, page 39-42
  • Meyer, G. and Corbett, J. D., "Reduced ternary halides of scandium: RbScX3 (X = chlorine, bromine) and CsScX3 (X = chlorine, bromine, iodine)", Inorganic Chemistry, 1981, volume 20, page 2627-31.
  • Corbett, J. D.; Daake, R. L.; Poeppelmeier, K. R. and Guthrie, D. H., "Metal-metal bonded clusters in transition metal Groups 3 and 4. Synthesis and structure of three M6 X12-type clusters for scandium and zirconium", Journal of the American Chemical Society, 1978, volume 100, page 652-4.
  • Poeppelmeier, K. R. and Corbett, J. D., "Metal-metal bonding in reduced scandium halides. Synthesis and crystal structure of scandium monochloride", Inorganic Chemistry, 1977, volume 16, page 294-7.



 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Scandium(III)_chloride". A list of authors is available in Wikipedia.
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