Electron affinities of halogens are in the order
Correct answer: B. Cl > F > Br > I
- A. F > Cl > Br > I
- B. Cl > F > Br > I
- C. Cl > Br > I > F
- D. Cl > Br > F > I
Explanation
The correct order of electron affinities for halogens is Cl > F > Br > I. Chlorine has the highest electron affinity among halogens due to its larger atomic size compared to fluorine, which reduces electron-electron repulsion in the added electron. Fluorine, although very electronegative, has a smaller atomic radius, resulting in increased electron-electron repulsion when an electron is added, making its electron affinity slightly less than that of chlorine. Bromine and iodine follow the expected trend of decreasing electron affinity as you move down the group due to increased atomic size and decreased nuclear attraction for the added electron.
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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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