Can you pls explain this paragraph??🙏 electrons and the exchange ener4T. Exchange energr is responsible
the stabilisation of ener4' state. Exchange energr is approximate I)
proportional to the total number of possible pairs of parallel
the degenerate orbitals. When several electrons occupy a set
degenerate orbitals, the lowest energy state corresponds to the maximum
possible extent of single occupation of orbital and parallel spins
rule). me loss of exchange energr increases the stability. As the
increases, the ionisation becomes more difficult. There is no loss
exchange energy at d configuration. Mn+ has 3d54s1 configuration
configuration of Cr+ is d, therefore, ionisation enthalpy of Mn+ is
than Cr+. In the same way. Fe2+ has d configuration and Mnl+ has 3
configuration. Hence, ionisation enthalpy of Fez + is lower than the
In other words, we can say that the third ionisation enthalpy of Fe
lower than that of Mn.
