Platinum hexafluoride is the chemical compound with the formula PtF6, and is one of seventeen known binary hexafluorides. 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 triplet ground state. PtF6 is a strong fluorinating agent and one of the strongest oxidants, capable of oxidising xenon and O2. PtF6 is octahedral in both the solid state and in the gaseous state. The Pt-F bond lengths are 185 picometers. Synthesis PtF6 was first prepared by reaction of fluorine with platinum metal. This route remains the method of choice. Pt + 3 F2 → PtF6 PtF6 can also be prepared by disproportionation of the pentafluoride (PtF5), with the tetrafluoride (PtF4) as a byproduct. The required PtF5 can be obtained by fluorinating PtCl2: 2 PtCl2 + 5 F2 → 2 PtF5 + 2 Cl2 2 PtF5 → PtF6 + PtF4 Hexafluoroplatinates Platinum hexafluoride can gain an electron to form the hexafluoroplatinate anion, . It is formed by reacting platinum hexafluoride with relatively uncationisable elements and compounds, for example with xenon to form "" (actually a mixture of , , and ), known as xenon hexafluoroplatinate. The discovery of this reaction in 1962 proved that noble gases form chemical compounds. Previous to the experiment with xenon, had been shown to react with oxygen to form [O2]+[PtF6]−, dioxygenyl hexafluoroplatinate. See also Hexafluoride Chloroplatinic acid References General reading Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. . Fluorides,6 Hexafluorides Platinum group halides Fluorinating agents Octahedral compounds Gases with color