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For large xenon, the attraction of electrons to the nucleus is weaker. It reacts with highly electronegative and little fluorine (and oxygen). Thus, the valence electron of $\mathbf{\text{Xe}}$is attracted to fluorine (or oxygen). This helps in the formation of compounds.

The powerful oxidizing agent ${\text{PtF}}_6$may oxidize xenon to create ${\text{XePtF}}_6$, an orange-yellow solid, since the ionization energy of oxygen $\left(1175\raisebox{1ex}{$\text{kJ}$}\!\left/ \!\raisebox{-1ex}{$\text{mol}$}\right.\right)$is extremely near to the initial ionization energy of xenon $\left(1170\raisebox{1ex}{$\text{kJ}$}\!\left/ \!\raisebox{-1ex}{$\text{mol}$}\right.\right)$. Other compounds such as ${\text{XeF}}_2{\text{,XeF}}_4{\text{,XeO}}_3\text{,}$and ${\text{XeO}}_4$are also created. As a result, xenon generates compounds with oxidation states ranging from $+2$to $+8$.

The size of the xenon is the same as that of oxygen. With fluorine and oxygen, xenon produces a variety of compounds.

Helium's initial ionization energies, Neon's $\left(2380\raisebox{1ex}{$\text{kJ}$}\!\left/ \!\raisebox{-1ex}{$\text{mol}$}\right.\right)$, and Argon's $\left(1520\raisebox{1ex}{$\text{kJ}$}\!\left/ \!\raisebox{-1ex}{$\text{mol}$}\right.\right)$are all higher than oxygen's first ionization energy.

It is possible to promote all role="math" localid="1663318478598" $s$and role="math" localid="1663318469688" $p$electrons to the vacant $d$orbitals. However, in the case of $\text{He}$and $\mathrm{Ne}$, the $d$orbital is absent.

The initial ionization energy of $\text{Kr}$is $1351\raisebox{1ex}{$\text{kJ}$}\!\left/ \!\raisebox{-1ex}{$\text{mol}$}\right.$which is possesses empty $d$orbitals.

As a result, $\text{Kr}$only forms a limited number of compounds.