Which of the following iso-electronic species has the highest IE?
Correct answer: D. Na+
- A. Ne
- B. F
- C. O2-
- D. Na+
Explanation
Ionization energy (IE) refers to the energy required to remove an electron from a gaseous atom or ion. For iso-electronic species, the one with the highest nuclear charge will have the highest ionization energy because the electrons are held more tightly. In this question, all species are iso-electronic with 10 electrons, but Na+ has the highest nuclear charge (+11) compared to Ne (neutral, +10), F (+9), and O2- (+8). Therefore, Na+ has the highest ionization energy among the given options. Ne follows, then F, and finally O2- due to increasing electron shielding and decreasing effective nuclear charge.
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About Periodic Properties and Trends
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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