Which of the following sets of elements would have nearly same atomic radii?
Correct answer: C. Fe, Co, Ni, Cu
- A. Na, K, Rb, Cs
- B. Na, Mg, Al, Si
- C. Fe, Co, Ni, Cu
- D. F, Cl, Br, I
Explanation
The correct answer is Option C: Fe, Co, Ni, Cu. These elements are transition metals located in the same period in the periodic table. In transition metals, the atomic radii tend to be similar due to the additional electron shielding effect, which reduces the effective nuclear charge experienced by the outer electrons. As a result, the atomic sizes of Fe, Co, Ni, and Cu are nearly the same. Option A is incorrect because Na, K, Rb, and Cs are alkali metals, and their atomic radii increase significantly as you move down the group. Option B is incorrect as Na, Mg, Al, and Si are in the same period, but their atomic radii decrease across the period from left to right. Option D is incorrect because F, Cl, Br, and I are halogens, and their atomic radii increase down the group.
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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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