An atom that is considered a "good" electron needs to have an available energy level that is lower than the energy of a valence electron of a different atom. An atom that is considered a "poor" electron will have the valence electrons be at a higher energy than other atoms. Given this, consider rows 2 and 5 in the periodic table. Why should fluorine, in row 2, be more reactive than iodine, in row 5, while lithium, in row 2, is less reactive than rubidium, in row 5?

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An atom that is considered a "good" electron needs to have an available energy level that is lower than the energy of a valence electron of a different atom. An atom that is considered a "poor" electron will have the valence 
electrons be at a higher energy than other atoms. Given this, consider rows 2 and 5 in the periodic table. 
Why should fluorine, in row 2, be more reactive than iodine, in row 5, while lithium, in row 2, is less reactive 
than rubidium, in row 5?

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