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• Exothermic reactions: lose energy and involve bonds breaking; ΔH is negative
• Endothermic reactions: gain energy and involve bonds forming; ΔH is positive
Recall that electron affinity is the energy change from the addition of 1 e– to a gaseous element/ion.
It is represented by this chemical equation:
Atom(g) + e– → Ion–(g), ΔE = –E.A.
The trend for electron affinity is as follows: it increases from left to right and decreases down a period in the periodic table.
For which element is the gaining of an electron most exothermic?
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