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
SMILES Cl[Sc](Cl)Cl
InChI InChI=1S/3ClH.Sc/h3*1H;/q;;;+3/p-3 Y Key: DVMZCYSFPFUKKE-UHFFFAOYSA-K Y 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
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
Y chloride (verify) (what is: Y/N?) 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.

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