Scandium chloride

Scandium(III) chloride
Names


IUPAC name Scandium(III) chloride
Other names scandium chloride scandium trichloride
Identifiers
CAS Number	10361-84-9
3D model (JSmol)	Interactive image
ChemSpider	74528^Y
ECHA InfoCard	100.030.714
PubChem CID	82586
RTECS number	VQ8925000
UNII	53PH22NTYW^Y
CompTox Dashboard (EPA)	DTXSID5042372
InChI InChI=1S/3ClH.Sc/h31H;/q;;;+3/p-3^Y Key: DVMZCYSFPFUKKE-UHFFFAOYSA-K^Y InChI=1/3ClH.Sc/h31H;/q;;;+3/p-3 Key: DVMZCYSFPFUKKE-DFZHHIFOAN InChI=1S/3ClH.Sc/h3*1H;/q;;;+3/p-3 Key: DVMZCYSFPFUKKE-UHFFFAOYSA-K
SMILES Cl[Sc](Cl)Cl
Properties
Chemical formula	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)
Solubility in water	70.2 g/100 mL
Solubility in other solvents	soluble in alcohol, acetone, glycerin insoluble in EtOH^{[citation needed]}
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	irritant
NFPA 704 (fire diamond)	1 0
Lethal dose or concentration (LD, LC):
LD₅₀ (median dose)	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). Y verify (what is ^YN ?) Infobox references

Chemical compound

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.

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

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 Sc^IICl₃⁻, containing Sc^IICl₆ octahedra sharing faces.^[10]

Uses

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

References

^ Frederikse, H.P.R.; Lide, David R. (1998). CRC Handbook of Chemistry and Physics (78th Edition)
^ ^a ^b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ 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
^ ^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
^ The Rare Earth Elements, Fundamentals and Applications David A. Atwood, 2012, John Wiley & Sons Inc, ISBN 9781119950974
^ Manzer, L. E., "Tetrahydrofuran Complexes of Selected Early Transition Metals", Inorganic Syntheses, 1982, volume 21, page 135-40.doi:10.1002/9780470132524.ch31
^ 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.
^ 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.
^ 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.
^ 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.
^ Metal Suppliers Online. (2000). Scandium Chloride