Which element having the following electronic configurations has the minimum ionization potential?

The first ionization enthalpies of $C$,$N$,and $F$ are $1086$,$1402$,and $1681 \, kJ \, mol^{-1}$ respectively. Which of the following values is the most likely first ionization enthalpy of $O$ ($1310$ or $1510 \, kJ \, mol^{-1}$)?

Given below are two statements $:$
Statement $(I) :$ The first ionisation enthalpy of group $14$ elements is higher than the corresponding elements of group $13.$
Statement $(II) :$ Melting points and boiling points of group $13$ elements are in general much higher than those of the corresponding elements of group $14.$ In the light of the above statements,choose the most appropriate answer from the options given below $:$

Starting from the $1^{st}$,the successive ionization potentials of an element are respectively $5.98, 18.8, 28.4, 120.1, 154 \ eV$. The element is

If first ionization enthalpy $(\Delta_i H)$ values of $Na$,$Mg$ and $Si$ are respectively $496$,$737$ and $786 \ kJ \ mol^{-1}$,the first ionization enthalpy value of $Al$ (in $kJ \ mol^{-1}$) will be

As one moves along a given row in the periodic table,ionization energy