Which of the following statement is correct ?
Correct answer: B. size of Na+ ion < Na atom
- A. size of Cl atoms > Cl- ion
- B. size of Na+ ion < Na atom
- C. size of Na atom < Na+ ion
- D. Cl- < Na+
Explanation
A sodium atom loses its outer electron to form Na+, so the ion has fewer electron shells and a smaller radius: Na+ is smaller than Na. In contrast, Cl− gains an electron and is larger than the neutral chlorine atom. Students may choose Cl− < Na+ by comparing nuclear charge only, but electron number and shell arrangement also control ionic size.
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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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