The increasing order of the first ionization enthalpies of the elements $B$,$P$,$S$ and $F$ (lowest first) is:

The incorrect order of $1^{st}$ $IP$ of the elements is

Which electronic configuration shows the minimum first ionisation energy?

The correct order of second $I.E.$ of $C$,$N$,$O$,and $F$ is:

The first ionisation potential of $Na$,$Mg$,$Al$ and $Si$ are in the order :-

Among the second period elements,the actual ionization enthalpies are in the order $Li < B < Be < C < O < N < F < Ne$. Explain why:
$(i)$ $Be$ has higher $\Delta_{i}H$ than $B$
$(ii)$ $O$ has lower $\Delta_{i}H$ than $N$ and $F$?