Scandium chloride

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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 Edit this at Wikidata
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,
glycerin
insoluble in EtOH[citation needed
]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 irritant
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability (yellow): no hazard codeSpecial hazards (white): no code
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 ?)

Scandium(III) chloride is the

hexahydrate
(ScCl3•6H2O) are commercially available.

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

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

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

lasers.[11]

References

  1. ^ Frederikse, H.P.R.; Lide, David R. (1998). CRC Handbook of Chemistry and Physics (78th Edition)
  2. ^
    ISBN 978-0-08-037941-8
    .
  3. doi:10.3891/acta.chem.scand.48-0294
  4. ^
    doi:10.1039/a803339k
  5. ^ The Rare Earth Elements, Fundamentals and Applications David A. Atwood, 2012, John Wiley & Sons Inc,
    ISBN 9781119950974
  6. doi:10.1002/9780470132524.ch31
  7. doi:10.1016/S0040-4020(99)00642-0
    .
  8. doi:10.1002/zaac.19372310107
    .
  9. doi:10.1021/ar00068a003
    .
  10. ISSN 0020-1669
    .
  11. ^ Metal Suppliers Online. (2000). Scandium Chloride


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