Question

Among the second period elements the actual ionization enthalpies are in the order Li < B < Be < C < O < N < F < Ne. Explain why

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?

What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?

The first ionization enthalpy values (in kJ mol–1) of group 13 elements are : | Element | B | Al | Ga | In | Tl | |---------|---|----|----|----|----| | Value | 801 | 577 | 579 | 558 | 589 | How would you explain this deviation from the general trend ?