| Gold(V) fluoride | |
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Gold(V) fluoride |
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Other names
gold pentafluoride |
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| Identifiers | |
| CAS number | 57542-85-5 |
| Properties | |
| Molecular formula | AuF5 |
| Molar mass | 291.959 g/mol |
| Appearance | red unstable solid |
| Melting point |
60 °C (Decomposes) |
| Solubility in water | Decomposes |
| Structure | |
| Crystal structure | orthorhombic (Pnma) |
| Hazards | |
| Main hazards | Corrosive, toxic |
| Related compounds | |
| Other cations | SbF5, BrF5, IF5 |
| Related compounds | AuF3 |
| (verify) (what is: /?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
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.
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]
This salt decomposes at 180 °C to produce the pentafluoride:
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