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Answer 1 · 2017-02-13T09:33:36

Note that iron is NOT a main group element, and thus it does not really follow the octet rule.

For iron, $Z=26$

The full electronic configuration of the iron atom is:

$1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^6$

OR $[Ar]4s^(2)3d^(6)$

As is standard for a transition metal, upon oxidation, the $4s$ electrons are removed FIRST to give $"ferrous ion"$ , $Fe^(2+)$ :

$1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^6$

And further oxidation can occur to give $"ferric ion"$ , $Fe^(3+)$ :

$1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^5$ .

In general, iron exhibits $Fe(II+)$ and $Fe(III+)$ oxidation states......