Along a period, atomic radius decreases. This gradual decrease in radius is due to:
Correct answer: B. Increase in number of protons in the nucleus
- A. Increase in number of electrons in valence shells
- B. Increase in number of protons in the nucleus
- C. Decrease in number of shells
- D. Increase in number of shells
Explanation
Along a period, the number of shells increases (electrons are added to the same principal energy level), and the atomic number increases. More protons attract the valence electrons. Electrons are gradually pulled closer to the nucleus because of the increased positive 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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