Q29 / 150 · MHT CET 2026 (17 April Shift 2) · Chemistry
Which of the following noble gases exhibits higher oxidation states ?
- ANe
- BAr
- CKr
- Correct answerDXe
Solution
As we move down the group of noble gases, the atomic size increases and the ionization enthalpy decreases.
Xenon has a relatively low ionization enthalpy, which allows its valence electrons to be excited to empty d-orbitals.
This enables Xenon to form compounds with highly electronegative elements like fluorine and oxygen.
Xenon exhibits higher oxidation states such as $+2$, $+4$, $+6$, and $+8$ in compounds like $\text{XeF}_2$, $\text{XeF}_4$, $\text{XeF}_6$, $\text{XeO}_3$, and $\text{XeO}_4$.
Neon and Argon do not form stable compounds, and Krypton only forms $\text{KrF}_2$ with an oxidation state of $+2$.
Therefore, Xenon exhibits higher oxidation states.
Answer: Xe
Xenon has a relatively low ionization enthalpy, which allows its valence electrons to be excited to empty d-orbitals.
This enables Xenon to form compounds with highly electronegative elements like fluorine and oxygen.
Xenon exhibits higher oxidation states such as $+2$, $+4$, $+6$, and $+8$ in compounds like $\text{XeF}_2$, $\text{XeF}_4$, $\text{XeF}_6$, $\text{XeO}_3$, and $\text{XeO}_4$.
Neon and Argon do not form stable compounds, and Krypton only forms $\text{KrF}_2$ with an oxidation state of $+2$.
Therefore, Xenon exhibits higher oxidation states.
Answer: Xe
Hence, the correct answer is option: 'D'.