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How would you explain the fact that the first ionization of Na is lower than that of Mg but its second ionization enthalpy is higher than that of Mg?

Monjur Alahi

How would you explain the fact that the first ionization of Na is lower than that of Mg but its second ionization enthalpy is higher than that of Mg?


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Salim Ahmed Kawsar

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The electronic configurations of Na and Mg are: Na:1s2 2s2 2p6 3s1 And Mg: 1s2 2s2 2p6 3s2 thus, the first electron in both the cases has to be removed from the 3s orbital, but the nuclear charge of Na is lower than that of Mg, therefore, the first ionization energy of Na is lower than that of Mg. But after the removal of the first electron, Na acquire the nearest noble gas configuration (Ne) which makes Na highly stable, but an electron is still left in the p orbital of Mg. Hence second ionization energy of Na is higher than that of Mg.

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