Four successive members of first row transition elements are listed below with their atomic numbers. Which one of them is expected to have the highest third ionization enthalpy:
Correct answer: C. Manganese (Z = 25)
- A. Iron (Z = 26)
- B. Chromium (Z = 24)
- C. Manganese (Z = 25)
- D. Vanadium (Z = 23)
Explanation
The third ionization enthalpy is the energy required to remove the third electron from a neutral atom. Manganese (Mn), with the configuration [Ar] 4s² 3d⁵, has a stable half-filled d-orbital. Disrupting this stable configuration requires a higher amount of energy compared to the other elements listed, as none of them are initially in a stable or half-filled state. Iron (Fe) and Chromium (Cr) do not lead to particularly stable configurations upon removal of the third electron, and Vanadium (V) becomes more stable upon losing the third electron. Therefore, Mn has the highest third ionization enthalpy among the given options.
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Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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