|various other names||Hexofluoroxenon|
|Molar mass||245.28 g mol-1|
|Density||3.56 g cm-3|
|Solubility in water||reacts v water|
|other than where noted otherwise, data are given for materials in their conventional state(at 25°C, 100kPa)Infobox disclaimer and references|
Xenon hexafluoride is the chemical compound v the formula XeF6. This colorless crystalline compound is just one of the three binary fluorides xenon, the various other two gift XeF2 and also XeF4. All space exergonic and also stable at common temperatures. XeF6 is the the strongest fluorinating certified dealer of the series.
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Xenon hexafluoride can be all set by permanent heating of XeF2 at around 300 degrees and pressure 6 MPa.
The framework of XeF6 forced several years to establish in contrast to the instances of xenon difluoride and xenon tetrafluoride. In the gas phase it adopts a slightly distorted octahedral geometry. The lacks perfect octahedral symmetry, as predicted by VSEPR theory because of the presence of 6 fluoride ligands and one lone pair the electrons. Follow to Konrad Seppelt, then Associate Professor of Chemistry at the university of Heidelberg, "the framework is ideal described in terms of a cell phone electron pair the moves end the faces and edges that the octahedron and also thus distorts the in a dynamic manner.".<1>NMR spectra of129Xe19F6 show that that is tetrameric: 4 equivalent xenon atoms are arranged in a tetrahedron surrounding by a fluctuating variety of 24 fluorine atoms the interchange location in a "cogwheel mechanism".
Xenon hexafluoride hydrolyzes stepwise, eventually affording xenon trioxide:<2>XeF6 + H2O → XeOF4 + 2 HFXeOF4 + H2O → XeO2F2 + 2 HFXeO2F2 + H2O → XeO3 + 2 HF
XeF6 serves as a Lewis acid, binding one and also two fluoride anions:XeF6 + F- → XeF7-XeF7- + F- → XeF82-
The two other binary fluorides carry out not form such stable adducts with fluoride. The salt Rb2XeF8 is amongst the many robust xenon compounds, decomposing only over 400 °C.
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