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Which one of the following is the reason behind fluorine having lower electron affinity than chlorine?
A
Smaller radius of fluorine, high electron density.
B
Smaller radius of chlorine, high electron density.
C
Bigger radius of fluorine, less electron density.
D
Smaller radius of chlorine, less electron density.
Explanation
Fluorine has a smaller atomic radius compared to chlorine, because as we move down a group, the atomic number increases causing the number of electrons and shells to increase. This results in an increase in atomic radius down the group. Because of this smaller radius, the electrons in fluorine are closer together and experience more repulsion from each other. When an additional electron is added to a fluorine atom, it experiences significant electron-electron repulsion due to the high electron density around the small fluorine nucleus. This repulsion makes it less energetically favorable for fluorine to gain an electron compared to chlorine, which has a larger atomic radius and thus lower electrons density, resulting in less repulsion. Thus, the high electron density around the small fluorine nucleus makes the electron affinity of fluorine lower than of chlorine.
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