Examples: XeF2, XeO3, XeOF2.
Xenon does not have to follow the octet rule because of its access to the 4d sublevel. The Lewis structure of XeO3 places a Xe in the center, double bonded to three O atoms and with one lone pair on the Xe.
Xenon have completely filled orbitals / energy levels. It has 8 valence electrons and have stable electronic configuration. Hence it is chemically inert and generally donot form compounds under normal conditions. However under high temperature and pressure, xenon combines with oxygen to form oxides like XeO3, XeO4 etc.
If you mean the equation for the production of NO from the elements at STP, it would be: N2 + O2 => 2NO OR ½N2 + ½O2 => NO
Noble gases are chemically inert and do not combine with alkaline earth metals. However, xenon will combine with highly electronegative elements like fluorine and oxygen forming compounds like XeO2, XeO3, XeF4, XeF6, XeOF4 etc.
The chemical name for XeO3 is xenon trioxide.
XeO3
XeO3
Formula: XeO3
XeO3 has two names under the IUPAC naming convention, xenon trioxide and xenon(VI) trioxide. This unstable compound is also known as xenic anhydride.
Examples: XeF2, XeO3, XeOF2.
XeF4+H2O->XeO3+HF+H2O
Xenon trioxide has a trigonal planar shape.
methane
Xenon does not have to follow the octet rule because of its access to the 4d sublevel. The Lewis structure of XeO3 places a Xe in the center, double bonded to three O atoms and with one lone pair on the Xe.
in XeO3 ,Xe shows sp3 but shape is pyramidal because of the presence of a lone pair of electrons on the central xenon atom. This lone pair distorts the shape of the molecule making it pyramidal.
Xenon Trioxide