On fluorine and other much more reactive species. Can we oxidize N2?

To set the stage we start with videos showing the extreme reactivity of F2. We then present insights into the chemical synthesis of fluorine which had long thought to be impossible. We proceed to the chemistry of the halogen fluorides and show examples of the chemistry of BrF5, explosions and peculiar novel anions we have obtained.

We venture on to platinum hexafluoride, which is known for its enormous oxidizing power. It gained its popularity mainly due to its ability to oxidize Xe, forming the first noble gas compound “XePtF6”. In addition to Xe, PtF6 is also able to oxidize various other compounds whose oxidation seemed impossible at the time. For example, NF3 or ClF5 can be oxidized to the coordinatively saturated cations [NF4]+ or [ClF6]+. However, the formation of [BrF6]+ by the reaction of BrF5 and PtF6 is not possible. To oxidize BrF5, even stronger oxidizing agents such as [KrF]+ or [NiF3]+ generated in situ are required.

We show that RuF6 is able to oxidize all known halogen pentafluorides XF5 (X = Cl, Br, I) at room temperature to the respective [XF6]+ salts and that it even oxidizes PtF4 and PtF5 back to PtF6. Therefore, RuF6 is more reactive than PtF6 under the investigated conditions.