Recall that electron affinity is the energy change from the addition of 1 e– to a gaseous element/ion.
Atom(g) + e– → Ion–(g), ΔE = –E.A. → more negative → most exothermic
It increases from left to right and decreases down a period in the periodic table.
Which electron affinity below would you predict to be the most exothermic?
(1) Al(g) + e− → Al–(g)
(2) N(g) + e− → N−(g)
(3) Ne(g) + e− → Ne−(g)
(4) Cl(g) + e− → Cl−(g)
(5) O−(g) + e− → O2−(g)
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