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Iron has an electronic configuration of [Ar] 3d6 4s2. Both outer shells (3 and 4 are incomplete - this is typical for the transition metals, and explained by the aufbau principle. In theory you would need an additional 4 electrons to fill the 3d shell (making it d10), and additionally 6 p electrons, 10 d electrons and 14 f electrons to fill the 4th

What happens in practise is the iron has common oxidation states of 2 (losing the 4s2 electrons) and 3 (additionally losing one d electron).

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