The noble gases have closed-shell electronic configuration and are monoatomic gases used normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.
The direct reaction of xenon with fluorine leads to a series of compounds with oxidation number +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.
The structure of XeO3 is
Xe is sp3 - hybridised, 3 Xe=O double bonds with one lone pair. The electron clouds on the atoms around the Xe and the lone pair of electrons will repel each other. As a result they will be pushed apart giving the XeO3 molecule a pyramidal molecular geometry or shape.