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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 ;
ECHA InfoCard	100.030.714
PubChem CID	82586;
RTECS number	VQ8925000;
UNII	53PH22NTYW ;
CompTox Dashboard (EPA)	DTXSID5042372 ;
	InChI InChI=1S/3ClH.Sc/h31H;/q;;;+3/p-3 Key: DVMZCYSFPFUKKE-UHFFFAOYSA-K ; 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) ; 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). verify (what is ?) 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] 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