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19 Nov 2019
Why does electron affinity tend to become more exothermic as you move right across a period? The trend in electron affinity is just the opposite of that for first ionization energy, since the two processes are the oppose of each other. As you move right across the period, you have a greater likelihood of pairing electrons in an orbital, which is a more stable configuration. As you move right across the period, metallic character decreases, meaning that the atom or ion is more likely to gain electrons than lose electrons. The effective nuclear charge increases as you move right across the period, resulting in greater attraction for an electron.
Why does electron affinity tend to become more exothermic as you move right across a period? The trend in electron affinity is just the opposite of that for first ionization energy, since the two processes are the oppose of each other. As you move right across the period, you have a greater likelihood of pairing electrons in an orbital, which is a more stable configuration. As you move right across the period, metallic character decreases, meaning that the atom or ion is more likely to gain electrons than lose electrons. The effective nuclear charge increases as you move right across the period, resulting in greater attraction for an electron.
Trinidad TremblayLv2
27 Mar 2019