Which of the following electronic configurations has the highest ionization enthalpy?

Ionisation energy in group $I$ elements varies in the decreasing order as:

Which of the following represents the correct order of first ionization enthalpy?
$(i) \ Li < B < Be < C$ $(ii) \ O < N < F$ $(iii) \ Be < N < Ne$

The successive ionization enthalpy values for an unknown element are $\Delta_i H_1 = 899 \ kJ/mol$,$\Delta_i H_2 = 1757 \ kJ/mol$,$\Delta_i H_3 = 14847 \ kJ/mol$,and $\Delta_i H_4 = 17948 \ kJ/mol$. To which group of the periodic table does this element belong?

The first three ionisation energies (in $kJ/mol$) of three representative elements are given below:

Element	$IE_1$	$IE_2$	$IE_3$
$P$	$495.8$	$4562$	$6910$
$Q$	$737.7$	$1451$	$7733$
$R$	$577.5$	$1817$	$2745$

Which of the following options is incorrect?

The first ionization enthalpies of $Be$,$B$,$N$ and $O$ follow the order...