why melting point of Mn is less than fe when fe has less no.of unpaired electrons
Dear Student,
Electronic configuration of Mn = [Ar] 3d5 4s2
Electronic configuration of Fe = [Ar] 3d6 4s2
In Mn, 3d shell is half filled and 4s shell in full filled which results in stable electronic configuration. Therefore, electrons are held tightly and there is less delocalisation of electrons which makes metallic bond weaker. On the contrary, Fe has only full filled 4s stability. The 3d is more than half filled and so the metallic bond formed is more stronger than that in Mn. The weaker the metallic bond, the less will be the melting point.Hence, melting point of Mn is less than Fe.
Electronic configuration of Mn = [Ar] 3d5 4s2
Electronic configuration of Fe = [Ar] 3d6 4s2
In Mn, 3d shell is half filled and 4s shell in full filled which results in stable electronic configuration. Therefore, electrons are held tightly and there is less delocalisation of electrons which makes metallic bond weaker. On the contrary, Fe has only full filled 4s stability. The 3d is more than half filled and so the metallic bond formed is more stronger than that in Mn. The weaker the metallic bond, the less will be the melting point.Hence, melting point of Mn is less than Fe.