What is the order of the first,second,and third ionization enthalpies of an element?

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 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:

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

The first ionization enthalpy values (in $kJ\,mol^{-1}$) of group $13$ elements are :

$B$	$801$
$Al$	$577$
$Ga$	$579$
$In$	$558$
$Tl$	$589$

How would you explain this deviation from the general trend?

The atomic numbers of elements $X, Y$,and $Z$ are $19, 37$,and $55$ respectively. Which of the following statements is correct?