 | |
 | |
| Names | |
|---|---|
| IUPAC name Platinum(VI) fluoride | |
| Other names Platinum hexafluoride | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider |
|
| ECHA InfoCard | 100.033.816 |
| EC Number |
|
| |
| |
| Properties | |
| PtF6 | |
| Molar mass | 309.07 g/mol |
| Appearance | dark-red crystals |
| Density | 3.83 g/cm3 |
| Melting point | 61.3 °C (142.3 °F; 334.4 K) |
| Boiling point | 69.14 °C (156.45 °F; 342.29 K) |
| Reacts with water | |
| Structure | |
| Orthorhombic,oP28 | |
| Pnma, No. 62 | |
| octahedral (Oh) | |
| 0 | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | Strong oxidizer |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Related compounds | Platinum(IV) fluoride Platinum(V) fluoride |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Platinum hexafluoride is thechemical compound with theformulaPtF6, and is one of seventeen known binaryhexafluorides. 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 isparamagnetic with atriplet ground state. PtF6 is a strong fluorinating agent and one of the strongest oxidants, capable of oxidising xenon and O2. PtF6 isoctahedral in both the solid state and in the gaseous state. The Pt-F bond lengths are 185picometers.[1]
PtF6 was first prepared by reaction of fluorine with platinum metal.[2] This route remains the method of choice.[1]
PtF6 can also be prepared bydisproportionation of the pentafluoride (PtF5), with the tetrafluoride (PtF4) as a byproduct. The required PtF5 can be obtained by fluorinating PtCl2:
Platinum hexafluoride can gain an electron to form thehexafluoroplatinate anion,PtF−
6. It is formed by reacting platinum hexafluoride with relatively uncationisable elements and compounds, for example withxenon to form "XePtF
6" (actually a mixture ofXeFPtF
5,XeFPt
2F
11, andXe
2F
3PtF
6), known asxenon hexafluoroplatinate. The discovery of this reaction in 1962 proved thatnoble gases form chemical compounds. Previous to the experiment with xenon,PtF
6 had been shown to react with oxygen to form [O2]+[PtF6]−,dioxygenyl hexafluoroplatinate.
