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Write electronic configurations of Fe, Fe2 + ,Fe3 + 

Answer
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Hint: We will determine the atomic number and write the electronic configuration of Fe metal. The superscript on the representation of the element symbol tells the oxidation number of the element. The oxidation number of an element tells the number of electrons gained or lost. The positive charge shows the loss of electrons. The negative charge shows the gain of electrons.

Complete step by step solution:The Fe metal belongs to the d-block. The electronic configuration of the d-block element is, (n1)d110ns.
It is a third period and eight group element. So, the outermost shell of Fe will be3d4s and the valence electron will be eight.
The atomic number of iron is 26.
So, the electronic configuration of Fe is as follows:

1s22s22p63s23p63d64s2
Fe is a neutral atom. The oxidation number of Fe in Fe2 + is +2 it means Fe loses two electrons. When it loses two electrons it formsFe2 + .
So, the electronic configuration of Fe2 + is as follows:
1s22s22p63s23p63d6
The oxidation number of Fe in Fe3 + is +3 it means Fe loses three electrons. When Fe loses three electrons it formsFe3 + .
So, the electronic configuration of Fe3 + is as follows:
1s22s22p63s23p63d5

Note: Block tells the outermost orbitals of the element and also tells the general configuration. The period number tells the principal quantum number of the outermost shell. Group number indicates the electrons present in the outermost valence shell. The group number can also be represented in roman numbers. S and P-block are represented by ‘A’ and the d-block is represented by ‘B’. The subscript on the representation of the element symbol tells the number of atoms.
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