In which of the following electronic configurations will there be a large difference between the second and third ionization energy?

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 $:$

The successive $5$ ionisation energies of an element are $800, 2427, 3658, 25024$ and $32824 \ kJ/mol$,respectively. By using the above values,predict the group in which the above element is present:

Given below are two statements:
Statement $I$: The first ionization energy of $Pb$ is greater than that of $Sn$.
Statement $II$: The first ionization energy of $Ge$ is greater than that of $Si$.
In the light of the above statements,choose the correct answer from the options given below:

Calculate the energy required to convert all atoms in $4.8 \ g$ of $Mg$ to $Mg^{2+}$ in the vapour state. $IE_1$ and $IE_2$ of $Mg$ are $740 \ kJ / mol$ and $1450 \ kJ / mol$ respectively.

The $1^{\text{st}}$,$2^{\text{nd}}$,and $3^{\text{rd}}$ ionization enthalpies $I_1, I_2$,and $I_3$ of four atoms with atomic numbers $n, n+1, n+2$,and $n+3$,where $n < 10$,are tabulated below. What is the value of $n$?

Atomic number	$I_1$ $(kJ/mol)$	$I_2$ $(kJ/mol)$	$I_3$ $(kJ/mol)$
$n$	$I_1$	$I_2$	$I_3$
$n+1$	$1681$	$3374$	$6050$
$n+2$	$2081$	$3952$	$6122$
$n+3$	$496$	$4562$	$6910$
$n+4$	$738$	$1451$	$7733$