Question

Why is second ionization enthalpy of sodium greater than its first ionization enthalpy?

Answer 1

Answer:

Explanation:

The first ionization energy of magnesium is larger than sodium because magnesium has one more proton in its nucleus to hold on to the electrons in the 3s orbital. ... The third ionization energy of magnesium is enormous, however, because the Mg2+ ion has a filled-shell electron configuration.

Answer 2

Explanation:

First ionisation enthalpy causes sodium to form Na+ from Na . As a result, one electron decreases and the orbits are more strongly attracted by the nucleus. It is evident that the atomic radius of a cation is always lesser than a neutral

atom as in that case, the orbits come closer due to less negative charge that has to be pulled.

Atomic radius of an atom is inversely proportional to ionisation enthalpy. So, now more energy has to be applied to make the valence electron free as the atomic radius becomes lesser than before.

That is why second ionisation enthalpy is greater than first ionisation enthalpy for sodium.

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