Oxygen’s ability to stabilize high oxidation states surpasses that of fluorine, as seen in the highest fluoride (MnF₄) and oxide (Mn₂O₇) of manganese, highlighting oxygen’s superiority in forming multiple bonds to metals.

The highest known oxide for iron is Fe₂O₃, and no higher oxides are known beyond Group 7. Although ferrates (VI) are formed in alkaline media, they readily decompose to Fe₂O₃ and O₂.

Oxygen’s ability to stabilize the highest oxidation state is evident in oxides, with the highest oxidation number coinciding with the group number, observed in Sc₂O₃ to Mn₂O₇.

The low third ionization enthalpy in Zn is due to the removal of one 4s electron, resulting in a stable d¹⁰ configuration. Removing electrons from d⁵ (Mn²⁺) and d¹⁰ (Zn²⁺) ions is challenging, leading to high third ionization enthalpies.

The high third ionization enthalpies of copper, nickel, and zinc indicate the difficulty in removing additional electrons, limiting their oxidation states to values not greater than two.

The low value for Sc reflects the stability of Sc³⁺, which possesses a noble gas configuration, highlighting the preference for achieving noble gas stability in its oxidation states.

The highest value for Zn is attributed to the removal of an electron from the stable d¹⁰ configuration of Zn²⁺, emphasizing the significance of achieving a fully filled d orbital for stability.

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.

Cr and Cu show high second ionization enthalpies due to the removal of electrons from d orbitals, resulting in d⁵ and d¹⁰ configurations in M²⁺ ions, influencing their stability.