$A$ sudden large jump between the values of second and third ionisation energies of an element would be associated with the electronic configuration:

Given below are two statements: One is labelled as Assertion $A$ and the other is labelled as Reason $R$.
Assertion $A$: The first ionization enthalpy of $O$ is lower than that of $N$ and $F$.
Reason $R$: The loss of an electron from $O$ leads to a stable half-filled $p$ orbital.
In light of the above statements, choose the most appropriate answer from the options given below:

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

The first ionization enthalpy $(\Delta_{i} H)$ values of the third period elements,$Na, Mg$ and $Si$ are respectively $496, 737$ and $786 \, kJ \, mol^{-1}$. Predict whether the first $\Delta_{i} H$ value for $Al$ will be more close to $575$ or $760 \, kJ \, mol^{-1}$? Justify your answer.

The first ionisation energy of $Na$,$B$,$N$ and $O$ atoms follows the order

The first ionization potentials in electron volts $(eV)$ of nitrogen and oxygen atoms are respectively given by: