Consider the elements $Ne$,$Na$,and $Mg$. The element with the highest first ionization enthalpy and the element with the lowest second ionization enthalpy,respectively,are:

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:

What is ionization enthalpy? What is the unit of ionization enthalpy?

In the long form of the periodic table,the elements having the lowest ionisation potentials are present in:

The sum of $IE_1 + IE_2$ and $IE_3 + IE_4$ for elements $P$ and $Q$ are given below:

Element	$IE_1 + IE_2$ $(kJ/mol)$	$IE_3 + IE_4$ $(kJ/mol)$
$P$	$2.45$	$8.82$
$Q$	$2.85$	$6.11$

Then,according to the given information,the incorrect statement$(s)$ is/are:

Which one of the following statements is incorrect in relation to ionisation enthalpy?