Problem: In the ground-state electron configuration of Fe3+, how many unpaired electrons are present? Express your answer numerically as an integer.Build the orbital diagram for the ion most likely formed by phosphorus.

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Iron (Fe) has an atomic number of 26. The ground state electron configuration of the Fe atom is:

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{6}$

With the ion $Fe^{3+}$ , iron has now lost 3 electrons to become more positive. Therefore, the ground state electron configuration of the $Fe^{3+}$ ion must also be missing those 3 electrons.

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In the ground-state electron configuration of Fe3+, how many unpaired electrons are present? Express your answer numerically as an integer.

Build the orbital diagram for the ion most likely formed by phosphorus.

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