Which of the following ions has smaller ionic radius?
Correct answer: D. Ti4+
- A. K+
- B. Ca2+
- C. Ti3+
- D. Ti4+
Explanation
The ionic radius of an ion depends on the number of electrons and the charge of the ion. As the positive charge on an ion increases, the ion loses more electrons and the effective nuclear charge experienced by the remaining electrons increases, pulling them closer to the nucleus and resulting in a smaller ionic radius. Ti4+ has the highest positive charge among the given ions, having lost four electrons, and thus has the smallest ionic radius. In contrast, K+, Ca2+, and Ti3+ have fewer lost electrons and larger ionic radii.
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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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