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{{Other uses|Gold fluoride}}
{{chembox
{{chembox
| verifiedrevid = 388262175
| verifiedrevid = 388262175
Line 9: Line 10:
|Section1={{Chembox Identifiers
|Section1={{Chembox Identifiers
| CASNo = 57542-85-5
| CASNo = 57542-85-5
| RTECS =
| ChEBI = 30080
| StdInChI=1S/Au.5FH/h;5*1H/q+5;;;;;/p-5
| StdInChIKey=QLYSAMSIXPXFDZ-UHFFFAOYSA-I
| SMILES=F[Au](F)(F)(F)F
| Gmelin = 1124345
| PubChem = 139033578
}}
}}
|Section2={{Chembox Properties
|Section2={{Chembox Properties
| Formula = AuF<sub>5</sub>
| Formula = Au<sub>2</sub>F<sub>10</sub>
| MolarMass = 291.959 g/mol
| MolarMass = 291.959 g/mol
| Appearance = red unstable solid
| Appearance = red unstable solid
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| MainHazards = Corrosive, toxic
| MainHazards = Corrosive, toxic
| FlashPt =
| FlashPt =
| RPhrases =
| SPhrases =
}}
}}
|Section8={{Chembox Related
|Section8={{Chembox Related
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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.


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; other pentafluorides are monomeric ([[Phosphorus pentafluoride|P]], [[Arsenic pentafluoride|As]], [[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>In-Chul Hwang, Konrad Seppelt "Gold Pentafluoride: Structure and Fluoride Ion Affinity" ''Angewandte Chemie International Edition'' 2001, volume 40, 3690-3693. {{doi|
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|
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.


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"/>


==Synthesis==
==Synthesis==
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}}</ref>
}}</ref>


:Au(s) + O<sub>2</sub>(g) + 3 F<sub>2</sub>(g) → O<sub>2</sub>AuF<sub>6</sub>(s)
:Au(s) + O<sub>2</sub>(g) + 3 F<sub>2</sub>(g) → O<sub>2</sub>AuF<sub>6</sub>(s)
This salt decomposes at 180&nbsp;°C to produce the pentafluoride:
This salt decomposes at 180&nbsp;°C to produce the pentafluoride:
: 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)
: 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)


[[Krypton difluoride]] is primarily a powerful oxidising and fluorinating agent. It can oxidise [[gold]] to its highest-known oxidation state, +5:<ref name="henderson">{{cite book
[[Krypton difluoride]] can also oxidise [[gold]] to the +5 oxidation state:<ref name="henderson">{{cite book
| title = Main group chemistry
| title = Main group chemistry
| author = W. Henderson
| author = W. Henderson
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{{Gold compounds}}
{{Gold compounds}}
{{Fluorine compounds}}


[[Category:Fluorides]]
[[Category:Fluorides]]
[[Category:Metal halides]]
[[Category:Metal halides]]
[[Category:Gold compounds]]
[[Category:Gold compounds]]
[[Category:Gold–halogen compounds]]

Latest revision as of 23:07, 28 May 2024

For other uses, see Gold fluoride.
Gold(V) fluoride
Gold(V) fluoride
Names
IUPAC name
Gold(V) fluoride
Other names
Gold pentafluoride
Perauric fluoride
Identifiers
3D model (JSmol)
ChEBI
1124345
  • InChI=1S/Au.5FH/h;5*1H/q+5;;;;;/p-5
    Key: QLYSAMSIXPXFDZ-UHFFFAOYSA-I
  • F[Au](F)(F)(F)F
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
 Corrosive, toxic
Related compounds
Other cations
 SbF5, BrF5, IF5
Related compounds
 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]
  1. ^ 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
  2. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  3. ^ Emeléus, H. J.; Sharpe, A. G. (1983). Advances in Inorganic Chemistry and Radiochemistry. Academic Press. p. 83. ISBN 0-12-023627-3.
  4. ^ W. Henderson (2000). Main group chemistry. Great Britain: Royal Society of Chemistry. p. 149. ISBN 0-85404-617-8.
  5. ^ 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.
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