Scandium(III) fluoride, ScF3, is an ionic compound. This salt is slightly soluble in water but dissolves in the presence of excess fluoride to form the ScF63− anion.[2]
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| Names | |
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| IUPAC name
Scandium(III) fluoride
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| Other names
Scandium trifluoride
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| Identifiers | |
3D model (JSmol)
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| ECHA InfoCard | 100.033.854 |
| EC Number |
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PubChem CID
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| RTECS number |
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CompTox Dashboard (EPA)
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| Properties | |
| ScF3 | |
| Molar mass | 101.95112 g/mol |
| Appearance | bright white powder |
| Density | 2.53 g/cm3 |
| Melting point | 1,552 °C (2,826 °F; 1,825 K)[2] |
| Boiling point | 1,607 °C (2,925 °F; 1,880 K)[2] |
Solubility product (Ksp)
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5.81×10−24[1] |
| Structure | |
| Cubic, Pm3m | |
| Pm3m, No. 221 | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other anions
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Scandium(III) chloride Scandium(III) bromide Scandium(III) iodide |
Other cations
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Yttrium(III) fluoride Lutetium(III) fluoride |
Related compounds
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Scandium(III) nitrate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Production
editScF3 can be produced by reacting scandium and fluorine.[3] It is also formed during the extraction from the ore thortveitite by the reaction of Sc2O3 with ammonium bifluoride at high temperature:[4]
- Sc2O3 + 6 NH4HF2 → 2 ScF3 + 6 NH4F + 3 H2O
The resulting mixture contains a number of metal fluorides and this is reduced by reaction with calcium metal at high temperature.[4] Further purification steps are required to produce usable metallic scandium.[4]
Properties
editScandium trifluoride exhibits the unusual property of negative thermal expansion, meaning it shrinks when heated. This phenomenon is explained by the quartic oscillation of the fluoride ions. The energy stored in the bending strain of the fluoride ion is proportional to the fourth power of the displacement angle, unlike most other materials where it is proportional to the square of the displacement. A fluorine atom is bound to two scandium atoms, and as temperature increases the fluorine oscillates more perpendicularly to its bonds. This motion draws the scandium atoms together throughout the bulk material, which contracts.[5] ScF3 exhibits this property from at least 10 K to 1100 K above which it shows the normal positive thermal expansion; furthermore, the material has cubic symmetry over this entire temperature range, and up to at least 1600 K at ambient pressure. The negative thermal expansion at very low temperatures is quite strong (coefficient of thermal expansion around -14 ppm/K between 60 and 110 K).[6]
At ambient pressures scandium trifluoride adopts the cubic crystal system, using the perovskite structure with one metal position vacant.[7] The unit cell dimension is 4.01 Å.[7] Under pressure scandium trifluoride also forms different crystal structures with rhombohedral, and above 3 GPa tetrahedral.[7]
Scandium fluoride (ScF₃) features high transparency across UV to IR wavelengths, low optical absorption, and a low refractive index (~1.5).[8][9] It exhibits nonlinear optical properties for frequency conversion and can luminesce when doped with rare-earth ions.[10]
References
edit- ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–189. ISBN 978-1138561632.
- ^ a b c Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier, ISBN 0-12-352651-5.
- ^ S.A.Cotton, Scandium, Yttrium and the Lanthanides: Inorganic and Coordination Chemistry, Encyclopedia of Inorganic Chemistry, 1994, John Wiley & Sons, ISBN 0-471-93620-0.
- ^ a b c Pradyot Patnaik, 2003, Handbook of Inorganic Chemicals, McGraw-Hill Professional, ISBN 0-07-049439-8.
- ^ Woo, Marcus (7 November 2011). "An incredible shrinking material: Engineers reveal how scandium trifluoride contracts with heat". Physorg. Retrieved 8 November 2011.
- ^ Greve, Benjamin K.; Kenneth L. Martin; Peter L. Lee; Peter J. Chupas; Karena W. Chapman; Angus P. Wilkinson (19 October 2010). "Pronounced Negative Thermal Expansion from a Simple Structure: Cubic ScF3". Journal of the American Chemical Society. 132 (44): 15496–15498. doi:10.1021/ja106711v. PMID 20958035.
- ^ a b c Aleksandrov, K. S.; V. N. Voronov; A. N. Vtyurin; A. S. Krylov; M. S. Molokeev; M. S. Pavlovskiĭ; S. V. Goryaĭnov; A. Yu. Likhacheva; A. I. Ancharov (2009). "Pressure-induced phase transition in the cubic ScF3 crystal". Physics of the Solid State. 51 (4): 810–816. Bibcode:2009PhSS...51..810A. doi:10.1134/S1063783409040295. ISSN 1063-7834. S2CID 119874020.
- ^ Loewen, Eric. "Scandium Fluoride: Properties, Applications, and Future Prospects". Stanford Advanced Materials. Retrieved Oct 16, 2024.
- ^ Karimov, Denis; Buchinskaya, Irina (2019). "Growth from the Melt and Properties Investigation of ScF3 Single Crystals". Crystals. 9 (7): 371. doi:10.3390/cryst9070371.
- ^ Pang, Min; Feng, Jing (2013). "Phase-tunable synthesis and upconversion photoluminescence of rare-earth-doped sodium scandium fluoride nanocrystals". CrystEngComm (35): 6901–6904. doi:10.1039/C3CE40849C.