The comparatively high value for Mn signifies the stability of Mn²⁺(d⁵), while the comparatively low value for Fe highlights the extra stability associated with Fe³⁺(d⁵), showcasing the influence of electron configurations on oxidation state stability.
How does the comparatively high value for Mn and the comparatively low value for Fe correlate with the stability of their respective oxidation states, Mn²⁺(d⁵) and Fe³⁺(d⁵)?
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The comparatively high value for manganese (Mn) in terms of second ionization enthalpy correlates with the stability of Mn²⁺, which possesses a d⁵ electron configuration. Mn²⁺ is particularly stable due to its half-filled d subshell. On the other hand, the comparatively low second ionization enthalpy for iron (Fe) corresponds to the extra stability of Fe³⁺, which has a d⁵ electron configuration. The stability of Fe³⁺ is attributed to achieving a half-filled d subshell, reinforcing the connection between ionization enthalpies and the stability of specific oxidation states in transition metals.