Which of the following noble gases exhibits h | vedclass

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(D) $1$. Noble gases are generally inert due to their stable electronic configuration.$2$. Among the noble gases, $Xe$ (Xenon) has the lowest ionizati

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$Xe$

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(D) $1$. Noble gases are generally inert due to their stable electronic configuration.$2$. Among the noble gases, $Xe$ (Xenon) has the lowest ionization enthalpy due to its large atomic size.$3$. Because of this, $Xe$ can easily form compounds with highly electronegative elements like $F$ and $O$, exhibiting higher oxidation states such as $+2, +4, +6,$ and $+8$ (e.g., in $XeF_6$ and $XeO_4$).

Which of the following noble gases exhibits higher oxidation states?

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