Gold(V) fluoride: Difference between revisions
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ratio 82:12 → ratio 82:18 (as per Hwang + Seppelt paper, p.3691) |
rv, compound is molecular and dimeric |
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{{Other uses|Gold fluoride}} |
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| verifiedrevid = 388262175 |
| verifiedrevid = 388262175 |
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| Name = Gold(V) fluoride |
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| ImageFile = Gold pentafluoride.png |
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| ImageName = Gold(V) fluoride |
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| IUPACName = Gold(V) fluoride |
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| OtherNames = Gold pentafluoride<br> Perauric fluoride |
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|Section1={{Chembox Identifiers |
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| CASNo = 57542-85-5 |
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| ChEBI = 30080 |
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| StdInChI=1S/Au.5FH/h;5*1H/q+5;;;;;/p-5 |
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| StdInChIKey=QLYSAMSIXPXFDZ-UHFFFAOYSA-I |
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| SMILES=F[Au](F)(F)(F)F |
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| Gmelin = 1124345 |
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| PubChem = 139033578 |
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|Section2={{Chembox Properties |
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| Formula = Au<sub>2</sub>F<sub>10</sub> |
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| MolarMass = 291.959 g/mol |
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| Appearance = red unstable solid |
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| Density = |
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| Solubility = Decomposes |
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| MeltingPtC = 60 |
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| MeltingPt = 60 °C (Decomposes) |
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| MeltingPt_notes = (decomposes) |
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|Section3={{Chembox Structure |
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| MolShape = |
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| Coordination = |
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| CrystalStruct = orthorhombic (Pnma) |
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| Dipole = |
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|Section7={{Chembox Hazards |
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| ExternalSDS = |
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| MainHazards = Corrosive, toxic |
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| FlashPt = |
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|Section8={{Chembox Related |
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| OtherCompounds = [[Gold(III) fluoride|AuF<sub>3</sub>]], [[Gold heptafluoride|AuF<sub>7</sub>]] |
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| OtherCations = [[Antimony pentafluoride|SbF<sub>5</sub>]], [[Bromine pentafluoride|BrF<sub>5</sub>]], [[Iodine pentafluoride|IF<sub>5</sub>]] |
| OtherCations = [[Antimony pentafluoride|SbF<sub>5</sub>]], [[Bromine pentafluoride|BrF<sub>5</sub>]], [[Iodine pentafluoride|IF<sub>5</sub>]] |
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'''Gold(V) fluoride''' is the [[inorganic compound]] with the formula Au<sub>2</sub>F<sub>10</sub>. This [[fluoride]] compound features [[gold]] in its highest known [[oxidation state]]. This red solid dissolves in [[hydrogen fluoride]] but these solutions decompose, liberating fluorine. |
'''Gold(V) fluoride''' is the [[inorganic compound]] with the formula Au<sub>2</sub>F<sub>10</sub>. This [[fluoride]] compound features [[gold]] in its highest known [[oxidation state]]. This red solid dissolves in [[hydrogen fluoride]] but these solutions decompose, liberating fluorine. |
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The structure of gold(V) fluoride in the solid state is [[centrosymmetric]] with hexacoordinated gold and an [[octahedral molecular geometry|octahedral arrangement]] of the fluoride centers |
The structure of gold(V) fluoride in the solid state is [[centrosymmetric]] with hexacoordinated gold and an [[octahedral molecular geometry|octahedral arrangement]] of the fluoride centers on each gold center. It is the only known dimeric pentafluoride, although sulfur can form [[disulfur decafluoride]]; other pentafluorides are monomeric ([[Phosphorus pentafluoride|P]], [[Arsenic pentafluoride|As]], [[Antimony pentafluoride|Sb]], [[Chlorine pentafluoride|Cl]], [[Bromine pentafluoride|Br]], [[Iodine pentafluoride|I]]), tetrameric ([[Niobium pentafluoride|Nb]], [[Tantalum pentafluoride|Ta]], [[Chromium pentafluoride|Cr]], [[Molybdenum pentafluoride|Mo]], [[Tungsten pentafluoride|W]], [[Technetium pentafluoride|Tc]], [[Rhenium pentafluoride|Re]], [[Ruthenium pentafluoride|Ru]], [[Osmium pentafluoride|Os]], [[Rhodium pentafluoride|Rh]], [[Iridium pentafluoride|Ir]], [[Platinum pentafluoride|Pt]]), or polymeric ([[Bismuth pentafluoride|Bi]], [[Vanadium pentafluoride|V]], [[Uranium pentafluoride|U]]).<ref name="hwang">In-Chul Hwang, Konrad Seppelt "Gold Pentafluoride: Structure and Fluoride Ion Affinity" ''Angewandte Chemie International Edition'' 2001, volume 40, 3690-3693. {{doi| |
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10.1002/1521-3773(20011001)40:19<3690::AID-ANIE3690>3.0.CO;2-5}}</ref> In the gas phase, a mixture of dimer and trimer in the ratio 82:18 has been observed. |
10.1002/1521-3773(20011001)40:19<3690::AID-ANIE3690>3.0.CO;2-5}}</ref> In the gas phase, a mixture of dimer and trimer in the ratio 82:18 has been observed. |
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Gold pentafluoride is the strongest known fluoride ion acceptor, exceeding the acceptor tendency of even [[antimony pentafluoride]]. |
Gold pentafluoride is the strongest known fluoride ion acceptor, exceeding the acceptor tendency of even [[antimony pentafluoride]]; and is also the strongest known [[Lewis acid]].<ref name="hwang"/> |
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==Synthesis== |
==Synthesis== |
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}}</ref> |
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:Au(s) + |
:Au(s) + O<sub>2</sub>(g) + 3 F<sub>2</sub>(g) → O<sub>2</sub>AuF<sub>6</sub>(s) |
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This salt decomposes at 180 |
This salt decomposes at 180 °C to produce the pentafluoride: |
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: 2 O<sub>2</sub>AuF<sub>6</sub>(s) |
: 2 O<sub>2</sub>AuF<sub>6</sub>(s) → Au<sub>2</sub>F<sub>10</sub> (s) + 2 O<sub>2</sub>(g) + F<sub>2</sub>(g) |
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[[Krypton difluoride]] |
[[Krypton difluoride]] can also oxidise [[gold]] to the +5 oxidation state:<ref name="henderson">{{cite book |
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| title = Main group chemistry |
| title = Main group chemistry |
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| author = W. Henderson |
| author = W. Henderson |
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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 gaseous krypton and fluorine:<ref>{{cite book |
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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{{Gold compounds}} |
{{Gold compounds}} |
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{{Fluorine compounds}} |
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[[Category:Fluorides]] |
[[Category:Fluorides]] |
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[[Category:Metal halides]] |
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[[Category:Gold compounds]] |
[[Category:Gold compounds]] |
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[[Category:Gold–halogen compounds]] |
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[[ar:فلوريد الذهب الخماسي]] |
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[[cs:Fluorid zlatičný]] |
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[[fa:فلورید طلا(V)]] |
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[[hr:Zlato(V)-fluorid]] |
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[[nl:Goud(V)fluoride]] |
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[[zh:五氟化金]] |
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Latest revision as of 23:07, 28 May 2024
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| Names | |
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| IUPAC name
Gold(V) fluoride
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| Other names
Gold pentafluoride
Perauric fluoride | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| 1124345 | |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| Au2F10 | |
| Molar mass | 291.959 g/mol |
| Appearance | red unstable solid |
| Melting point | 60 °C (140 °F; 333 K) (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 |
Related compounds
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AuF3, AuF7 |
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 on each gold center. It is the only known dimeric pentafluoride, although sulfur can form disulfur decafluoride; 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 82:18 has been observed.
Gold pentafluoride is the strongest known fluoride ion acceptor, exceeding the acceptor tendency of even antimony pentafluoride; and is also the strongest known Lewis acid.[1]
Synthesis
[edit]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 can also oxidise gold to the +5 oxidation state:[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
[edit]- ^ a b 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.