Electron affinity decreases down the group because:
Correct answer: B. Atomic radius increases
- A. Proton number increases
- B. Atomic radius increases
- C. Shielding decrease
- D. Atomic radius decreases
Explanation
As atomic size increases, the electrons become further away from the nucleus and hence, electron affinity decreases. Another factor which affects electron affinity is effective nuclear charge, which is defined as the positive force experienced by electrons due to the pull of the positively charged nucleus.
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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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