In The Ground-state Electron Configuration Of fe3+, How Many Unpaired Electrons Are Present? Find Out Here.

The atomic number of iron (fe) is 26. Electronic configuration of Fe with 26 electrons is

1S2

2S2

2P6

3S2

3P6

4S2

3d6

Fe3+ means 926-3) electrons = 23 electrons.

Due to the fact partially filled orbital configuration is stable enough,

We can say

Fe3+ = 1s2  2s2 2p6 3s2 3p6 4do 3d5

The outer s and d orbitals dictates its configuration that orbitals therefore have 5 electrons in its outermost part. Since the outermost shell can be occupied by a maximum number of 10 electrons it will have 5 unpaired electrons.

Also

Fe-1s2 2s2 2p6 3s2 3p6 3d6 4s2

When Fe+ loses one electron = 1s2 2s2 2p6 3s2 3p6 3d6, 4s1

And when Fe loses 2 electrons, Fe2+ =1s2 2s2 2p6 3s2 3p6 3d6 4s0

When Fe loses 3 electrons its, Fe3+ =1s2 2s2 2p6 3s2 3p6 3d5

For Fe to convert to Fe3+ it will have to lose 2 electrons from 4s orbital and 1 electron from 3d orbital. The resulting electronic configuration becomes 4s^0 and 3d^5.

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