IRON SHOW +6 OXIDATION STATE BUT NOT +5 WHY ?
For higher oxidation states, transition metals use their ns e-s+(n-1)d unpaired electrons. since in the middle of the series there are maximum no. of unpaired electrons, elements show maximum oxidation state.
Since Fe has 4s2 3d6 configuration, it can show maximum oxidation state upto +6 due to 4 unpaired electrons.
On going down the group, the stability of higher oxidation state increases because ionization energy required to form +8 oxidation state is less for lower elements. Hence they can use all the 8 electrons for bonding.
Since Fe has 4s2 3d6 configuration, it can show maximum oxidation state upto +6 due to 4 unpaired electrons.
On going down the group, the stability of higher oxidation state increases because ionization energy required to form +8 oxidation state is less for lower elements. Hence they can use all the 8 electrons for bonding.