Which of the following configurations represents atoms of the elements having the highest second ionization energy?

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

Generally,the first ionization energy increases along a period. But there are some exceptions. One which is not an exception is

For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below:

$I.E.$	$1^{st}$	$2^{nd}$	$3^{rd}$	$4^{th}$	$5^{th}$
Value	$577.5$	$1810$	$2750$	$11580$	$14820$

The element is:

The first ionization energy of magnesium is smaller as compared to that of elements $X$ and $Y$,but higher than that of $Z$. The elements $X$,$Y$ and $Z$,respectively,are :

The atomic numbers of vanadium $(V)$,chromium $(Cr)$,manganese $(Mn)$,and iron $(Fe)$ are $23$,$24$,$25$,and $26$ respectively. Which one of these is expected to have the highest second ionization enthalpy?