Group 18 Xenon Compounds

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Noble gases were long thought inert, yet xenon forms compounds like XeF_2 and XeF_4; why can xenon react while helium and neon cannot?

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The reactivity of noble gases depends on how readily their valence electrons can be involved in bonding. Xenon, being a heavy noble gas, has a relatively low ionization enthalpy because its outer electrons are far from the nucleus and well shielded, and it has accessible empty d-orbitals that allow it to expand its octet and form bonds with highly electronegative elements like fluorine and oxygen. This is why xenon forms fluorides such as XeF_2 and XeF_4. Helium and neon, by contrast, are very small with extremely high ionization enthalpies and no accessible d-orbitals, so they remain chemically inert. The option that xenon is the smallest noble gas is false, since it is among the largest. The option that xenon is a metal is incorrect. The option that helium has more electrons is wrong, as helium has only two. This explanation of xenon's reactivity is a standard NCERT Group 18 topic. Understanding group 18 xenon compounds in this way ties directly into the wider study of p-block elements, where the same reasoning recurs across many problems. Plausibility check: only the heavier, low-ionization-enthalpy noble gases form compounds, matching the known chemistry of xenon and krypton, confirming the reasoning.

Group 18 Xenon Compounds

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