How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
The first ionization enthalpy of sodium is decrease than that of magnesium. This is mostly due to reasons: 1. The atomic length of sodium is extra than that of magnesium 2. The powerful nuclear rate of magnesium is better than that of sodium For those reasons, the power required to get rid of an electron from magnesium is extra than the power required in sodium. Hence, the primary ionization enthalpy of sodium is decrease than that of magnesium. However, the second one ionization enthalpy of sodium is better than that of magnesium. This is due to the fact after dropping an electron, sodium attains the strong noble fueloline configuration. On the opposite hand, magnesium, after dropping an electron nevertheless has one electron withinside the 3s-orbital. In order to gain the solid noble fueloline configuration, it nevertheless has to lose one extra electron. Thus, the strength required to get rid of the second one electron in case of sodium is lots better than that required in case of magnesium. Hence, the second one ionization enthalpy of sodium is better than that of magnesium.
