Gold(V) fluoride: Difference between revisions
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: 7 {{chem|KrF|2}} (g) + 2 Au (s) → 2 KrF{{su|p=+}}AuF{{su|b=6|p=−}} (s) + 5 Kr (g) |
: 7 {{chem|KrF|2}} (g) + 2 Au (s) → 2 KrF{{su|p=+}}AuF{{su|b=6|p=−}} (s) + 5 Kr (g) |
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KrF{{su|p=+}}AuF{{su|b=6|p=−}} decomposes at 60°C into gold(V) fluoride and krypton and fluorine |
KrF{{su|p=+}}AuF{{su|b=6|p=−}} decomposes at 60°C into gold(V) fluoride and gaseous krypton and fluorine:<ref>{{cite book |
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| title = Elements of the ''p'' block |
| title = Elements of the ''p'' block |
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| author = Charlie Harding |
| author = Charlie Harding |
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: KrF{{su|p=+}}AuF{{su|b=6|p=−}} → {{chem| |
:2 KrF{{su|p=+}}AuF{{su|b=6|p=−}} → {{chem|Au|2|F|10}} (s) + 2 Kr (g) + 2 {{chem|F|2}} (g) |
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==References== |
==References== |
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Revision as of 19:41, 28 June 2012
| |
| Names | |
|---|---|
| IUPAC name
Gold(V) fluoride
| |
| Other names
Gold pentafluoride
Perauric fluoride | |
| Identifiers | |
CompTox Dashboard (EPA)
|
|
| 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
|
Corrosive, toxic |
| Related compounds | |
Other cations
|
SbF5, BrF5, IF5 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
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, Sb, 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 dioxygenyl hexafluoroaurate:[2][3]
- Au(s) + O2(g) + 3 F2(g) → O2AuF6(s)
This salt decomposes at 180 °C to produce the pentafluoride:
- 2 O2AuF6(s) → Au2F10 (s) + 2 O2(g) + F2(g)
Krypton difluoride is primarily a powerful oxidising and fluorinating agent. It can oxidise gold to its highest-known oxidation state, +5:[4]
- 7 KrF
2 (g) + 2 Au (s) → 2 KrF+
AuF−
6 (s) + 5 Kr (g)
KrF+
AuF−
6 decomposes at 60°C into gold(V) fluoride and gaseous krypton and fluorine:[5]
- 2 KrF+
AuF−
6 → Au
2F
10 (s) + 2 Kr (g) + 2 F
2 (g)
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 0-12-023627-3.
- ^ W. Henderson (2000). Main group chemistry. Great Britain: Royal Society of Chemistry. p. 149. ISBN 0-85404-617-8.
- ^ Charlie Harding; David Arthur Johnson; Rob Janes (2002). Elements of the p block. Great Britain: Royal Society of Chemistry. p. 94. ISBN 0-85404-690-9.