Which of the following has the highest ionization energy?
Correct answer: D. P
- A. Al
- B. S
- C. Si
- D. P
Explanation
Phosphorus (P) has the highest ionization energy among the options given because it is located in group 15 of period 3, where ionization energy increases due to a higher effective nuclear charge and smaller atomic radius compared to the other elements listed.Aluminum (Al) has the lowest ionization energy because it is in group 13. Silicon (Si) has a higher ionization energy than aluminum but is still lower than phosphorus because it is further left in the periodic table. Sulfur (S), while having a higher ionization energy than silicon and aluminum, does not exceed that of phosphorus due to its position in group 16, which is still to the left of phosphorus.
This question appeared on the NUMS 2019 (cancelled sitting) paper, which you can sit online with every answer explained.
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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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