| Revision as of 12:35, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,055 edits Saving copy of the {{chembox}} taken from revid 473604549 of page Platinum_hexafluoride for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 09:44, 9 November 2024 edit 2401:d800:5df4:a140:847a:8ce8:8c1c:b336 (talk)No edit summaryTags: Mobile edit Mobile web edit |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{chembox |
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{{chembox |
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| verifiedrevid = 470456570 |
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| verifiedrevid = 476995092 |
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| ImageFile = PtF6.png |
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| ImageFile = PtF6.png |
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| ImageSize = 180px |
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| ImageSize = 180px |
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| IUPACName = Platinum hexafluoride |
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| ImageFile2=Platinum-hexafluoride-3D-vdW.png |
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| OtherNames = Platinum(VI) fluoride |
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| IUPACName = Platinum(VI) fluoride |
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| OtherNames = Platinum hexafluoride |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/6FH.Pt/h6*1H;/q;;;;;;+2/p-6 |
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| StdInChI = 1S/6FH.Pt/h6*1H;/q;;;;;;+2/p-6 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = NHVLQWBIZQMDAU-UHFFFAOYSA-H |
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| StdInChIKey = NHVLQWBIZQMDAU-UHFFFAOYSA-H |
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| SMILES = F(F)(F)(F)(F)F |
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| SMILES = F(F)(F)(F)(F)F |
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| InChI = 1S/6FH.Pt/h6*1H;/q;;;;;;+2/p-6 |
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| InChI = 1S/6FH.Pt/h6*1H;/q;;;;;;+2/p-6 |
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| InChIKey1 = NHVLQWBIZQMDAU-UHFFFAOYSA-H |
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| InChIKey1 = NHVLQWBIZQMDAU-UHFFFAOYSA-H |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo_Ref = {{cascite|changed|??}} |
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| CASNo = |
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| CASNo = 13693-05-5 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} |
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| ChemSpiderID=21106464 |
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| ChemSpiderID = 2283064 |
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| EINECS = 237-214-0 |
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| PubChem = 22238670 |
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}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = PtF<sub>6</sub> |
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| Formula = PtF<sub>6</sub> |
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| MolarMass = 309.07 g/mol |
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| MolarMass = 309.07 g/mol |
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| Appearance = dark-red crystals |
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| Appearance = dark-red crystals |
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| Density = 3.83 g/cm<sup>3<sup> |
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| Density = 3.83 g/cm<sup>3</sup> |
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| MeltingPt = 61.3 °C |
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| MeltingPtC = 61.3 |
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| BoilingPt = 69.14 °C |
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| BoilingPtC = 69.14 |
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| Solubility = reacts violently |
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| Solubility = Reacts with water |
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}} |
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| Section3 = {{Chembox Structure |
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|Section3={{Chembox Structure |
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| CrystalStruct = ], ] |
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| CrystalStruct = ], ] |
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| SpaceGroup = Pnma, No. 62 |
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| SpaceGroup = Pnma, No. 62 |
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| Coordination = octahedral (''O<sub>h</sub>'') |
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| Coordination = octahedral (''O<sub>h</sub>'') |
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| Dipole = 0 |
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| Dipole = 0 |
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| Section7 = {{Chembox Hazards |
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|Section7={{Chembox Hazards |
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| MainHazards = oxidizer |
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| MainHazards = Strong oxidizer |
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| NFPA-H = 4 |
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| NFPA-F = 0 |
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| NFPA-R = 4 |
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| NFPA-S = OX |
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| FlashPt = |
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| FlashPt = |
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| Autoignition = |
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| AutoignitionPt = |
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|Section8={{Chembox Related |
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| OtherCompounds = ] <br/> ] |
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'''Platinum hexafluoride''' is the ] with the ] ]], and is one of seventeen known binary ]s. It is a dark-red volatile solid that forms a red gas. The compound is a unique example of platinum in the +6 oxidation state. With only four d-electrons, it is ] with a ] ground state. PtF<sub>6</sub> is a strong fluorinating agent and one of the strongest oxidants, capable of oxidising xenon and O<sub>2</sub>. PtF<sub>6</sub> is ] in both the solid state and in the gaseous state. The Pt-F bond lengths are 185 ]s.<ref name=Seppelt/> |
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==Synthesis== |
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PtF<sub>6</sub> was first prepared by reaction of fluorine with platinum metal.<ref>{{cite journal | last1 = Weinstock | first1 = B. | last2 = Claassen | first2 = H. H. | last3 = Malm | first3 = J. G. | year = 1957 | title = Platinum Hexafluoride | journal = Journal of the American Chemical Society | volume = 79 | issue = 21| pages = 5832 | doi = 10.1021/ja01578a073 }}</ref> This route remains the method of choice.<ref name=Seppelt>{{cite journal | doi = 10.1021/ic052029f | title = Solid State Molecular Structures of Transition Metal Hexafluorides | date = 2006 | last1 = Drews | first1 = Thomas | last2 = Supeł | first2 = Joanna | last3 = Hagenbach | first3 = Adelheid | last4 = Seppelt | first4 = Konrad | journal = Inorganic Chemistry | volume = 45 | issue = 9 | pages = 3782–3788 | pmid = 16634614 }}</ref> |
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:Pt + 3 F<sub>2</sub> → PtF<sub>6</sub> |
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PtF<sub>6</sub> can also be prepared by ] of the pentafluoride (]), with the tetrafluoride (]) as a byproduct. The required PtF<sub>5</sub> can be obtained by fluorinating PtCl<sub>2</sub>: |
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:2 PtCl<sub>2</sub> + 5 F<sub>2</sub> → 2 PtF<sub>5</sub> + 2 Cl<sub>2</sub> |
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:2 PtF<sub>5</sub> → PtF<sub>6</sub> + PtF<sub>4</sub> |
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==Hexafluoroplatinates== |
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Platinum hexafluoride can gain an electron to form the ] anion, {{chem|Pt|F|6|-}}. It is formed by reacting platinum hexafluoride with relatively uncationisable elements and compounds, for example with ] to form "{{chem|Xe|Pt|F|6}}" (actually a mixture of {{chem|Xe|F|Pt|F|5}}, {{chem|Xe|F|Pt|2|F|11}}, and {{chem|Xe|2|F|3|Pt|F|6}}), known as ]. The discovery of this reaction in 1962 proved that ]es form chemical compounds. Previous to the experiment with xenon, {{chem|Pt|F|6}} had been shown to react with oxygen to form <sup>+</sup><sup>−</sup>, ]. |
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==See also== |
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* ] |
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* ] |
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==References== |
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{{reflist}} |
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== General reading == |
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* Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}. |
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{{Platinum compounds}} |
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{{Hexafluorides}} |
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{{fluorine compounds}} |
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] |
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] |
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] |
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] |
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] |
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] |