noble gases

Question

Noble gases have the highest ionization energies in their respective periods because:

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**Noble Gases** (Group 18) possess a highly stable closed-shell electronic configuration ($ns^2 np^6$).
- Every orbital is completely filled, leading to a state of **maximum stability** and symmetry.
- Removing an electron from such a stable configuration is extremely unfavorable and requires a massive amount of energy.
- Furthermore, they have the smallest atomic radius in their respective periods, maximizing the nuclear pull on valence electrons.

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