Gold(V) fluoride: Difference between revisions
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Revision as of 07:32, 21 May 2010
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| Names | |
|---|---|
| IUPAC name
Gold(V) fluoride
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| Other names
gold pentafluoride
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| Identifiers | |
CompTox Dashboard (EPA)
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| Properties | |
| AuF5 | |
| Molar mass | 291.959 g/mol |
| Appearance | red unstable solid |
| Melting point | 60 °C (Decomposes) |
| Decomposes | |
| Structure | |
| orthorhombic (Pnma) | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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Corrosive, toxic |
| Related compounds | |
Other cations
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SbF5, BrF5, IF5 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Gold(V) fluoride is the inorganic compound with the formula Au2F10. This fluoride compound features gold in its highest known oxidation state. This red solid dissolves in hydrogen fluoride but these solutions decompose, liberating fluorine.
The structure of gold(V) fluoride in the solid state is centrosymmetric with hexacoordinated gold and an octahedral arrangement of the fluoride centers around each gold center. It is the only known dimeric pentafluoride; other pentafluorides are monomeric (P, As, Cl, Br, I), tetrameric (Nb, Ta, Cr, Mo, W, Tc, Re, Ru, Os, Rh, Ir, Pt), or polymeric (Bi, V, U).[1] In the gas phase, a mixture of dimer and trimer in the ratio 82:12 has been observed.
Gold pentafluoride is the strongest known fluoride ion acceptor, exceeding the acceptor tendency of even antimony pentafluoride.
Synthesis
Gold(V) fluoride can be synthesized by heating gold metal in an atmosphere of oxygen and fluorine to 370 °C at 8 atmospheres to form gold dioxygenyl fluoride:[2][3]
- 2 Au + 2 O2 + 6 F2 → 2 O2AuF6
This salt decomposes at 180 °C to produce the pentafluoride:
- 2 O2Au2F6 → Au2F10 + 2 O2 + F2
References
- ^ In-Chul Hwang, Konrad Seppelt "Gold Pentafluoride: Structure and Fluoride Ion Affinity" Angewandte Chemie International Edition 2001, volume 40, 3690-3693. doi:10.1002/1521-3773(20011001)40:19<3690::AID-ANIE3690>3.0.CO;2-5
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Emeléus, H. J.; Sharpe, A. G. (1983). Advances in Inorganic Chemistry and Radiochemistry. Academic Press. p. 83. ISBN 0120236273.