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Fluorine, though higher than chlorine in the periodic table, has a very small atomic size. This makes the fluoride anion so formed unstable (highly reactive) due to a very high charge/mass ratio. As a result, fluorine has an electron affinity less than that of chlorine.
Fluorine is kind of an exception to the general rule of electron affinity. Typically, you would expect F to have a higher electron affinity since it is higher in the group than Cl. F is very small though, so there is electron-electron repulsion when you add a new electron because there are already electrons tightly held by the nucleus. Therefore, the electron affinity is lower than Cl due to the lessened attraction felt by the incoming electron.
shouse1I wrote:are electron affinity and electronegativity related?
They are related in the sense that they follow the same periodic trend. The highest electronegative and highest electron affinity are on the top right side of the periodic table. However, the noble gases are an exception in electron affinity as they have a full shell.
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