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{{Other uses|Gold fluoride}} |
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{{chembox |
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{{chembox |
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| verifiedrevid = 388262175 |
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| Name = Gold(V) fluoride |
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| ImageFile = Gold pentafluoride.png |
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| Name = Gold(V) fluoride |
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| ImageFile = Gold pentafluoride.png |
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<!-- | ImageSize = 200px --> |
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| ImageName = Gold(V) fluoride |
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| ImageName = Gold(V) fluoride |
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| IUPACName = Gold(V) fluoride |
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| IUPACName = Gold(V) fluoride |
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| OtherNames = gold pentafluoride |
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| OtherNames = Gold pentafluoride<br> Perauric fluoride |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo = 57542-85-5 |
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| CASNo = 57542-85-5 |
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| RTECS = |
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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(F)(F)(F)F |
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| Gmelin = 1124345 |
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| PubChem = 139033578 |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = AuF<sub>5</sub> |
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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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| MolarMass = 291.959 g/mol |
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| Appearance = red unstable solid |
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| Appearance = red unstable solid |
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| Density = |
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| Density = |
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| Solubility = Decomposes |
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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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}} |
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| Section3 = {{Chembox Structure |
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|Section3={{Chembox Structure |
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| MolShape = |
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| MolShape = |
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| Coordination = |
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| Coordination = |
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| CrystalStruct = orthorhombic (Pnma) |
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| CrystalStruct = orthorhombic (Pnma) |
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| Dipole = |
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| Dipole = |
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}} |
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}} |
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| Section7 = {{Chembox Hazards |
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|Section7={{Chembox Hazards |
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| ExternalMSDS = |
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| ExternalSDS = |
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| MainHazards = Corrosive, toxic |
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| MainHazards = Corrosive, toxic |
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| FlashPt = |
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| FlashPt = |
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| RPhrases = |
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| SPhrases = |
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}} |
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}} |
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| Section8 = {{Chembox Related |
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|Section8={{Chembox Related |
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| OtherCpds = ] |
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| OtherCompounds = ], ] |
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| OtherCations = ], ], ] |
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| OtherCations = ], ], ] |
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'''Gold(V) fluoride''' is the ] with the formula Au<sub>2</sub>F<sub>10</sub>. This ] compound features ] in its highest known ]. This red solid dissolves in ] but these solutions decompose, liberating fluorine. |
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'''Gold(V) fluoride''' is the ] with the formula Au<sub>2</sub>F<sub>10</sub>. This ] compound features ] in its highest known ]. This red solid dissolves in ] but these solutions decompose, liberating fluorine. |
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The structure of gold(V) fluoride in the solid state is ] with hexacoordinated gold and an ] 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).<ref>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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The structure of gold(V) fluoride in the solid state is ] with hexacoordinated gold and an ] of the fluoride centers on each gold center. It is the only known dimeric pentafluoride, although sulfur can form ]; other pentafluorides are monomeric (], ], ], ], ], ]), tetrameric (], ], ], ], ], ], ], ], ], ], ], ]), or polymeric (], ], ]).<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 82:12 has been observed. |
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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. |
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Gold pentafluoride is the strongest known fluoride ion acceptor, exceeding the acceptor tendency of even ]. |
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Gold pentafluoride is the strongest known fluoride ion acceptor, exceeding the acceptor tendency of even ]; and is also the strongest known ].<ref name="hwang"/> |
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==Synthesis== |
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==Synthesis== |
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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 ] fluoride:<ref>{{Greenwood&Earnshaw}}</ref><ref>{{cite book |
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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 ] hexafluoroaurate:<ref>{{Greenwood&Earnshaw}}</ref><ref>{{cite book |
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| title = Advances in Inorganic Chemistry and Radiochemistry |
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| title = Advances in Inorganic Chemistry and Radiochemistry |
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| first1 = H. J. |
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| first1 = H. J. |
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| publisher = Academic Press |
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| publisher = Academic Press |
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| year = 1983 |
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| year = 1983 |
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| isbn = 0120236273 |
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| isbn = 0-12-023627-3 |
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| page = 83 |
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| page = 83 |
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}}</ref> |
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}}</ref> |
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:2 Au + 2 O<sub>2</sub> + 6 F<sub>2</sub> → 2 O<sub>2</sub>AuF<sub>6</sub> |
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: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 °C to produce the pentafluoride: |
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This salt decomposes at 180 °C to produce the pentafluoride: |
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: 2 O<sub>2</sub>AuF<sub>6</sub> → Au<sub>2</sub>F<sub>10</sub> + 2 O<sub>2</sub> + F<sub>2</sub> |
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: 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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] can also oxidise ] to the +5 oxidation state:<ref name="henderson">{{cite book |
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| title = Main group chemistry |
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| author = W. Henderson |
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| location = Great Britain |
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| publisher = Royal Society of Chemistry |
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| year = 2000 |
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| isbn = 0-85404-617-8 |
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| page = 149 |
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}}</ref> |
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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) |
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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 |
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| title = Elements of the ''p'' block |
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| author = Charlie Harding |
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| author2 = David Arthur Johnson |
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| author3 = Rob Janes |
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| location = Great Britain |
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| publisher = Royal Society of Chemistry |
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| year = 2002 |
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| isbn = 0-85404-690-9 |
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| page = 94 |
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}}</ref> |
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: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== |
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==References== |
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{{Gold compounds}} |
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{{Gold compounds}} |
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{{Fluorine compounds}} |
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