Platinum hexafluoride 2498708 221437464 2008-06-24T14:19:57Z Puppy8800 5404759 iw {{Chembox new | ImageFile = PtF6.png | ImageSize = 200px | IUPACName = Platinum hexafluoride | OtherNames = Platinum(VI) fluoride | Section1 = {{Chembox Identifiers | CASNo = }} | Section2 = {{Chembox Properties | Formula = PtF6 | MolarMass = 309.1 | Appearance = red | Density = 5.21 | MeltingPt = 61.3 °C<ref name=Handbook>Perry, Dale L. and Sidney L. Phillips. <u>Handbook of Inorganic Compounds.<u> CRC Press, 1995. ISBN 0849386713. [http://books.google.com/books?id=0fT4wfhF1AsC&pg=PA297&lpg=PA297&dq=%22platinum+hexafluoride%22+boiling+point&source=web&ots=EAMQZ-tC6r&sig=hdeIN4EnUZgQwXOewyrdtgVLVBk Google Book Search Result]</ref> | BoilingPt = 69.1 °C<ref name=Handbook>Perry, Dale L. and Sidney L. Phillips. <u>Handbook of Inorganic Compounds.<u> CRC Press, 1995. ISBN 0849386713. [http://books.google.com/books?id=0fT4wfhF1AsC&pg=PA297&lpg=PA297&dq=%22platinum+hexafluoride%22+boiling+point&source=web&ots=EAMQZ-tC6r&sig=hdeIN4EnUZgQwXOewyrdtgVLVBk Google Book Search Result]</ref> | Solubility = }} | Section3 = {{Chembox Hazards | MainHazards = oxidizer | FlashPt = n.a. | Autoignition = n.a. }} }} '''Platinum hexafluoride''' is the [[chemical compound]] with the [[chemical formula|formula]] [[Platinum|Pt]][[Fluorine|F<sub>6</sub>]]. 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 paramagnetic with a [[spin triplet|triplet]] ground state. PtF<sub>6</sub> is a strong oxidant and a strong fluorinating agent that is best known for its reaction with [[xenon]] to form "XePtF<sub>6</sub>," known as [[xenon hexafluoroplatinate]]. The discovery of this reaction in 1962 proved that [[noble gas]]es form chemical compounds. Previous to the experiment with xenon, PtF<sub>6</sub> had been shown to react with oxygen to form (O<sub>2</sub>)<sup>+</sup>(PtF<sub>6</sub>)<sup>&minus;</sup>, [[dioxygen hexafluoroplatinate]]. ==Synthesis== PtF<sub>6</sub> was first prepared by reaction of fluorine with platinum metal.<ref>Weinstock, B.; Claassen, H. H.; Malm, J. G. “Platinum Hexafluoride” Journal of the American Chemical Society 1957, volume 79, pp 5832 - 5832. {{DOI|10.1021/ja01578a073}}</ref> This route remains the method of choice.<ref name=Seppelt>Drews, T.; Supel, J.; Hagenbach, A.; Seppelt, K. “Solid State Molecular Structures of Transition Metal Hexafluorides” Inorganic Chemistry 2006, volume 45, pp 3782-3788.{{DOI|10.1021/ic052029f}}</ref> :Pt + 3 F<sub>2</sub> → PtF<sub>6</sub> PtF<sub>6</sub> can also be prepared by [[disproportionation]] of PtF<sub>5</sub>. The required PtF<sub>5</sub> can be obtained by fluorinating PtCl<sub>2</sub> :PtCl<sub>2</sub> + 2.5 F<sub>2</sub> → PtF<sub>5</sub> + Cl<sub>2</sub> :2 PtF<sub>5</sub> → PtF<sub>6</sub> + PtF<sub>4</sub> ==Other hexafluoride compounds== The neutral hexafluorides of other elements are also volatile. These include [[osmium]], [[iridium]], [[rhodium]], [[ruthenium]], [[rhenium]], [[tungsten]], [[technetium]], and [[uranium]]. All are aggressive oxidants. [[Uranium hexafluoride]] and [[tungsten hexafluoride]] are used in the nuclear and microelectronics industries, respectively. In the main group elements, [[sulfur]], [[xenon]], [[selenium]], and [[tellurium]] form isolable hexafluorides. [[Sulfur hexafluoride]] is so extremely stable, perhaps due to [[steric effects]], that it is used as an inert fluid in transformers. The analogues [[selenium hexafluoride]] and [[tellurium hexafluoride]] are, however, strongly reactive. Like the hexafluorides of Mo, Tc, Ru, Rh, W, Re, Os, and Ir, PtF<sub>6</sub> is [[octahedral]] in both the solid state and in the gaseous state. The Pt-F bond lengths are 185 [[picometer]]s.<ref name=Seppelt/> ==References== <references/> ==General reading== * Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5. [[Category:Fluorides]] [[Category:Platinum compounds]] [[Category:Metal halides]] [[ja:六フッ化白金]] [[zh:六氟化铂]]