Platinum hexafluoride
Names | |
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IUPAC name
Platinum(VI) fluoride
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Other names
Platinum hexafluoride
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Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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100.033.816 |
EC Number |
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PubChem CID
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CompTox Dashboard (EPA)
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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
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Pnma, No. 62 | |
octahedral (Oh) | |
0 | |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards
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Strong oxidizer |
NFPA 704 (fire diamond) | |
Related compounds | |
Related compounds
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Platinum(V) fluoride
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Platinum hexafluoride is the
Synthesis
PtF6 was first prepared by reaction of fluorine with platinum metal.[2] This route remains the method of choice.[1]
- 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, PtF−
6. It is formed by reacting platinum hexafluoride with relatively uncationisable elements and compounds, for example with xenon to form "XePtF
6" (actually a mixture of XeFPtF
5, XeFPt
2F
11, and Xe
2F
3PtF
6), known as xenon hexafluoroplatinate. The discovery of this reaction in 1962 proved that noble 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.
See also
References
- ^
- .
General reading
- Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.