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lower than that of magnesium but its second ionization enthalpy is higher than
that of magnesium?
Asked by Dev Last Modified
Answer 
Vishaka Bhutia
Home Tutor
The first ionization enthalpy of sodium is lower than that of magnesium. This is primarily because of two reasons:
The atomic size of sodium is greater than that of magnesium
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.
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