The correct order of ionisation energy is:

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(D) The second ionization energy $(IE_2)$ refers to the energy required to remove an electron from a unipositive ion $(M^{+})$. The stability of the r

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$Mn^{+} < Fe^{+} < Cr^{+} < Co^{+}$

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(D) The second ionization energy $(IE_2)$ refers to the energy required to remove an electron from a unipositive ion $(M^{+})$. The stability of the resulting $M^{2+}$ ion and the electronic configuration of the $M^{+}$ ion play a crucial role.The electronic configurations of the $M^{+}$ ions are:$Cr^{+} (3d^5)$ - This is a stable half-filled configuration.$Mn^{+} (3d^5 4s^1)$$Fe^{+} (3d^6 4s^1)$$Co^{+} (3d^7 4s^1)$Due to the extra stability of the $3d^5$ configuration in $Cr^{+}$,removing the second electron from $Cr^{+}$ requires significantly higher energy compared to the others. The experimental values for $IE_2$ are approximately:$Mn^{+} \approx 1509 \, kJ/mol$$Fe^{+} \approx 1563 \, kJ/mol$$Co^{+} \approx 1644 \, kJ/mol$$Cr^{+} \approx 1591 \, kJ/mol$Comparing these values,the order is $Mn^{+} < Fe^{+} < Cr^{+} < Co^{+}$.

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