The first ionization enthalpy of sodium is more than that of magnesium. This is primarily

because of two reasons:

a. The atomic size of sodium is greater than that of magnesium

b. The effective nuclear charge of magnesium is higher than that of sodium

For these reasons, the energy required to remove an electron from magnesium is more

than the energy required in sodium. Hence, the first ionization enthalpy of sodium is lower

than that of magnesium.

However, the second ionization enthalpy of sodium is higher than that of magnesium. This

is because after losing an electron, sodium attains the stable noble gas configuration. On

the other hand, magnesium, after losing an electron still has one electron in the 3s-orbital.

In order to attain the stable noble gas configuration, it still has to lose one more electron.

Thus, the energy required to remove the second electron in case of sodium is much higher

than that required in case of magnesium. Hence, the second ionization enthalpy of sodium

is higher than that of magnesium.