Oxidizing agents platinum hexafluoride

Platinum hexafluoride does not have many commercial apphcations. It is used as a strong oxidizing agent and can oxidize oxygen from the air. It is used in research. Platinum hexafluoride forms compounds with molecular oxygen and xenon, [02" ][PtF6 ] and XePtFe, respectively. 

The hexafluoride is a very powerful oxidizing agent reacting violently with most oxidizable substances. Reaction with liquid water is violent forming HF, oxygen, lower fluorides of platinum, and other products. In vapor phase hydrolysis occurs more smoothly. 

In the early 1960s Neil Bartlett was studying the properties ot platinum hex-alluoride. an extremely powerful oxidizing agent. In fact, by merely mixing dioxygen with plaiinum hexafluoride, it is possible to remove one electron from the oxygen molecule and isolate the product ... 

Binary Compounds. Three fluorides, PtF4 [13455-15-7], PtF5 [37782-184-8], and platinum hexafluoride [136934)5-5], PtF., are well documented. The last is a powerful oxidizing agent and can oxidize dioxygen and xenon (235). Two chlorides exist, platinum dichloride [10025-65-7],... 

The same authors showed that platinum hexafluoride, which is a somewhat weaker oxidative fluorinating agent than KrF+, can also oxidize NF3, though the yield and purity of the NF4+ fluoroplatinate formed as a dark red solid were low. The pure salt was prepared for purposes of comparison by the thermal reaction at 125°C between NF3, F2, and PtF6. The reaction between NF3 and the hexafluoride was carried out either in HF solution at 25°C or under ultraviolet irradiation in the gas phase, also at ambient temperature. In each case the vibrational spectrum of the product showed the presence of a tetraflu-oroammonium salt, but the product was a mixture of fluoroplatinate and polyfluoroplatinate which could not be purified by extraction with liquid HF. 

Platinum(V) fluoride is a tetramer (structurally like 22.5) PtFg is a red solid and has a molecular structure consisting of octahedral molecules neutron powder diffraction data confirm little deviation from an ideal octahedral structure. The hexafluoride is a very powerful oxidizing agent (equation 22.127, and see Section 5.16) and attacks glass. The oxidizing power of the second row rZ-block hexafluorides... 

Note that diatomic oxygen is being oxidized by the platinum hexafluoride. The latter must indeed be a strong oxidizing agent. 

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