Lutetium(III) fluoride
(Redirected from Lutetium fluoride)
-fluorid.png)
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| Names | |
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| Other names
lutetium trifluoride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.033.945 |
| EC Number |
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PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| LuF3 | |
| Molar mass | 231.97g/mol[1] |
| Appearance | white powder[1] |
| Density | 8.29 g/cm3[1] |
| Melting point | 1,184[2] °C (2,163 °F; 1,457 K) |
| Boiling point | 2200°C[1] |
| n/a[1] | |
| Hazards | |
| GHS labelling: | |
 
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| Danger | |
| H301, H311, H315, H319, H331, H335 | |
| P261, P264, P270, P271, P280, P301+P310, P302+P352, P304+P340, P305+P351+P338, P311, P312, P321, P322, P330, P332+P313, P337+P313, P361, P362, P363, P403+P233, P405, P501 | |
| Related compounds | |
Other anions
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Lutetium(III) chloride Lutetium(III) bromide |
Other cations
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Scandium(III) fluoride Yttrium(III) fluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lutetium(III) fluoride is an inorganic compound with a chemical formula LuF3.
Production
[edit]Lutetium(III) fluoride can be produced by reacting lutetium oxide with hydrogen fluoride, or reacting lutetium chloride and hydrofluoric acid:[3]
- Lu2O3 + 6 HF → 2 LuF3 + 3 H2O
- LuCl3 + 3 HF → LuF3 + 3 HCl
It can also be produced by reacting lutetium sulfide and hydrofluoric acid:[4]
- 3 Lu
2S
3+ 20 HF + (2 + 2x) H
2O → 2 (H
3O)Lu
3F
10·xH
2O↓ + 9 H
2S↑ (x = 0.9) - (H3O)Lu3F10 → 3 LuF3 + HF↑ + H2O↑
Lutetium oxide and nitrogen trifluoride react at 240 °C to produce LuOF. A second step happens below 460 °C to produce LuF3.[5]
References
[edit]- ^ a b c d e "Lutetium Fluoride".
- ^ K.M Lyapunov, A.V Baginskii, S.V Stankus (June 2004). "Experimental study of the enthalpy of lutetium trifluoride in solid and liquid states". Journal of Alloys and Compounds. 372 (1–2): 7–9. doi:10.1016/j.jallcom.2003.09.139.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ Georg Brauer (ed.), In collaboration with Marianne Baudler u. a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 254.
- ^ O.V. Andrrev, I.A. Razumkova, A.N. Boiko (March 2018). "Synthesis and thermal stability of rare earth compounds REF 3 , REF 3 · n H 2 O and (H 3 O)RE 3 F 10 · n H 2 O (RE = Tb − Lu, Y), obtained from sulphide precursors". Journal of Fluorine Chemistry. 207: 77–83. doi:10.1016/j.jfluchem.2017.12.001.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ Randall D. Scheele, Bruce K. McNamara, Andrew M. Casella, Anne E. Kozelisky, Doinita Neiner (February 2013). "Thermal NF3 fluorination/oxidation of cobalt, yttrium, zirconium, and selected lanthanide oxides". Journal of Fluorine Chemistry. 146: 86–97. doi:10.1016/j.jfluchem.2012.12.013.
{{cite journal}}: CS1 maint: multiple names: authors list (link)
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