i believe this is the reasoning, if someone can confirm or deny this it would be appreciated...
Cr is in the
ground state and when we make elements and fill orbitals we follow the (n+ℓ
rule
(n+ℓ
rule: (fill lower energy orbitals first)
~FILLING: electrons fill orbitals with lower energy (n+ℓ
before filling orbitals with higher energy (n+ℓ
~if both the (n+ℓ
values are the same then the lower n value gets filled first
4s = (n+ℓ
= (4 +0) = 4
3d = (n+ℓ
= (3 + 2) = 5
~~prior to being filled the 4s orbital has lower energy than the 3d orbital
we know that once the exception transition metals (Cr,Mo and Cu,Ag) are formed and in their ground state, they prefer to have the max number of half-filled or fully-filled orbitals
so they promote an electron from the 4s orbital into a 3d orbital which creates an ideal situation (either half-filled or fully-filled orbitals)
sɐǝɹǝɥʍ
Fe2+ is an
ion and has lost 2 electrons
while the (n+ℓ
rule enabled us to see which orbital had higher energy, in these cases its only prior to them being filled
~LEAVING: in cation formation electrons leave orbitals of higher energy prior to leaving orbitals of lesser energy
~~once filled the 4s orbital is higher energy than the 3d orbital (4s orbital will be the outermost orbital)