Tantalum(V) fluoride
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| Names | |
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| Other names
tantalum pentafluoride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.029.111 |
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PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| TaF5 | |
| Molar mass | 275.93990 g·mol−1 |
| Appearance | white powder |
| Density | 4.74 g/cm3, solid |
| Melting point | 96.8 °C (206.2 °F; 369.9 K) |
| Boiling point | 229.5 °C (445.1 °F; 502.6 K) |
| decomposes | |
| +795.0·10−6 cm3/mol | |
| Structure | |
| 0 D | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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HF source |
| GHS labelling:[1] | |
 
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| Danger | |
| H302, H314 | |
| P260, P261, P264, P270, P271, P280, P301+P312, P301+P330+P331, P302+P352, P303+P361+P353, P304+P312, P304+P340, P305+P351+P338, P310, P312, P321, P322, P330, P363, P405, P501 | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
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Other cations
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Related compounds
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Tungsten hexafluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Tantalum(V) fluoride is the inorganic compound with the formula TaF5. It is one of the principal molecular compounds of tantalum. Characteristic of some other pentafluorides, the compound is volatile but exists as a tetramer in the solid state.
Preparation and structure
[edit]TaF5 is prepared by treating tantalum metal with fluorine gas.[2]
- 2 Ta + 5 F2 → 2 TaF5
NbF5 is prepared similarly.
Solid and molten TaF5 is tetrameric, consisting of four octahedral TaF6 centers linked via bridging fluoride centers. Gaseous TaF5 is monomeric and adopts the trigonal bipyramidal structure with D3h symmetry.[3]
Reactions and derivatives
[edit]The tendency of TaF5 to form clusters in the solid state indicates the Lewis acidity of the monomer. Indeed, TaF5 reacts with fluoride sources to give the ions [TaF6]− (hexafluorotantalate(V)), [TaF7]2− (heptafluorotantalate(V)), and [TaF8]3− (octafluorotantalate(V)). With neutral Lewis bases, such as diethyl ether, TaF5 forms adducts.
TaF5 is used in combination with HF as a catalyst for the alkylation of alkanes and alkenes and for the protonation of aromatic compounds. The TaF5–HF system is stable in reducing environments, unlike SbF5–HF.[4] In the presence of fluoride, tantalum pentafluoride forms the anions [TaF8]3−, [TaF7]2−, or [TaF6]−, depending on the nature of the counterion and the concentration of HF. High concentrations of HF favor the hexafluoride by virtue of the formation of [HF2]−:[5]
- [TaF7]2− + HF ⇌ [TaF6]− + [HF2]−
The salts M3TaF8 have been crystallized. For M = K, the crystals consist of [TaF7]2− anions together with fluoride that does not coordinate to Ta(V),[6] and the salt is actually potassium fluoride heptafluorotantalate(V) (K+)3[TaF7]2−F−. For M = Na, the crystals features [TaF8]3−,[7] and the salt is sodium octafluorotantalate(V) (Na+)3[TaF8]3−.
Section of the Na3[TaF8] structure (Ta = turquoise, F = green).
Relevance to separation of Ta and Nb
[edit]In the Marignac process, Nb and Ta are separated by fractional crystallization of K2[TaF7] from solutions of hydrofluoric acid. Under these conditions, niobium forms K2[NbOF5], which is more soluble than K2[TaF7]. Reduction of K2[TaF7] with sodium gives metallic Ta.[8]
References
[edit]- ^ "Tantalum pentafluoride". pubchem.ncbi.nlm.nih.gov. Retrieved 16 December 2021.
- ^ Priest, Homer F.; Swinehert, Carl F. (1950-01-01), Audrieth, Ludwig F. (ed.), "Anhydrous Metal Fluorides", Inorganic Syntheses, vol. 3 (1 ed.), Wiley, pp. 171–183, doi:10.1002/9780470132340.ch47, ISBN 978-0-470-13162-6, retrieved 2024-01-22
{{citation}}: ISBN / Date incompatibility (help) - ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Arpad Molnar; G. K. Surya Prakash; Jean Sommer (2009). Superacid Chemistry (2nd ed.). Wiley-Interscience. p. 60. ISBN 978-0-471-59668-4.
- ^ Anatoly Agulyanski (2004). The chemistry of tantalum and niobium fluoride compounds. Amsterdam: Elsevier. p. 134. ISBN 0-444-51604-2.
- ^ Ľubomír Smrčok; Radovan Černý; Miroslav Boča; Iveta Macková; Blanka Kubíková (2010). "K3TaF8 from Laboratory X-ray powder data". Acta Crystallographica C. 66 (2): pi16 – pi18. Bibcode:2010AcCrC..66I..16S. doi:10.1107/S0108270109055140. PMID 20124670.
- ^ Langer, V.; Smrčok, L.; Boča, M. (2010). "Redetermination of Na3TaF8". Acta Crystallographica C. 66 (9): pi85 – pi86. Bibcode:2010AcCrC..66I..85L. doi:10.1107/S0108270110030556. PMID 20814090.
- ^ Klaus Andersson, Karlheinz Reichert, Rüdiger Wolf "Tantalum and Tantalum Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH. Weinheim. doi:10.1002/14356007.a26_071