Chemistry

Question Analysis
This question involves comparing ionization energies of isoelectronic species (same electron configuration).
The main focus is on how nuclear charge affects ionization energy for particles with identical electron arrangements.

Key Concept Explanation
For isoelectronic ions/atoms, ionization energy increases with increasing nuclear charge (number of protons).
A higher nuclear charge exerts a stronger attraction on the same set of electrons, making it harder to remove an electron.

Step-by-Step Solution
1. Confirm all species are isoelectronic: Na⁺, Mg²⁺, Al³⁺, and F⁻ all have the [Ne] electron configuration (10 electrons).
2. Identify the nuclear charge (proton count) of each:
Na⁺: 11 protons
Mg²⁺: 12 protons
Al³⁺: 13 protons
F⁻: 9 protons
3. Relate nuclear charge to ionization energy: Hig...