Platinum hexafluoride

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Platinum hexafluoride
IUPAC name

Platinum hexafluoride

Other names

Platinum(VI) fluoride

Identifiers

 ChemSpider 21106464 YesY
Jmol-3D images {{#if:F[Pt-4](F)(F)(F)(F)F|Image 1
Properties
Molecular formula PtF6
Molar mass 309.07 g/mol
Appearance dark-red crystals
Density 3.83 g/cm3
Melting point 61.3 °C
Boiling point 69.14 °C
Solubility in water reacts violently
Structure
Crystal structure Orthorhombic, oP28
Space group Pnma, No. 62
Coordination
geometry		 octahedral (Oh)
Dipole moment 0
Hazards
Main hazards oxidizer
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Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Platinum hexafluoride is the chemical compound with the formula PtF6. 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 oxidant and a strong fluorinating agent. PtF6 is octahedral in both the solid state and in the gaseous state. The Pt-F bond lengths are 185 picometers.[1]

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 PtF5. 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

  1. ↑ 1.0 1.1 Drews, T.; Supel, J.; Hagenbach, A.; Seppelt, K. “Solid State Molecular Structures of Transition Metal Hexafluorides” Inorganic Chemistry 2006, volume 45, pp 3782-3788.doi:10.1021/ic052029f
  2. ↑ Weinstock, B.; Claassen, H. H.; Malm, J. G. “Platinum Hexafluoride” Journal of the American Chemical Society 1957, volume 79, pp 5832 - 5832. doi:10.1021/ja01578a073

General reading

  • Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
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