![Xenon element card: symbol Xe, atomic number 54, atomic mass 131.29, electron configuration [Kr] 4d¹⁰ 5s² 5p⁶, oxidation states +6 +4 +2, Noble gas, group 18, period 5, gas at room temperature.](https://stage.chemistry-dictionary.com/wp-content/uploads/2026/09/xenon-chemical-element.webp)
Xenon securely occupies group 18 of the standard periodic table of elements. It remains a highly unreactive noble gas under normal temperature and pressure conditions. This extreme stability occurs because it has a complete and stable valence electron shell.
Valence electrons are the outermost electrons that are involved in forming new chemical bonds. Despite its general inertness, the relatively large size of the xenon atom matters. Its outermost electrons are held less tightly by the distant atomic nucleus.
This looser grip allows xenon to undergo chemical reactions under specific extreme conditions. It primarily reacts with highly electronegative elements like pure fluorine and oxygen gas. This produces stable chemical compounds like xenon hexafluoroplatinate (XePtF6) and xenon tetrafluoride (XeF4).
Xenon naturally exists as a single-atom monatomic gas under standard laboratory conditions. It exhibits a characteristic, piercing blue glow when excited by an electrical discharge in a vacuum tube. Industrial companies commercially obtain it by the fractional distillation of supercooled liquid air.
This complex process makes xenon quite expensive due to its extreme scarcity in our atmosphere. Because of its high mass and density, xenon serves as an exceptionally efficient spacecraft propellant. Scientists frequently use it to power the ion thrusters used in deep space exploration satellites.