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

Assertion : Element has a tendency to lose the electron$(s)$ to attain the stable configuration.
Reason : Ionization enthalpy is the energy released to remove an electron from an isolated gaseous atom in its ground state.

If first ionization enthalpy $(\Delta_i H)$ values of $Na$,$Mg$ and $Si$ are respectively $496$,$737$ and $786 \ kJ \ mol^{-1}$,the first ionization enthalpy value of $Al$ (in $kJ \ mol^{-1}$) will be

Consider the following changes:
$M_{(s)} \to M_{(g)}$ ........$(1)$
$M_{(s)} \to M^{2+}_{(g)} + 2e^-$ .......$(2)$
$M_{(g)} \to M^{+}_{(g)} + e^-$ .........$(3)$
$M^{+}_{(g)} \to M^{2+}_{(g)} + e^-$ .........$(4)$
$M_{(g)} \to M^{2+}_{(g)} + 2e^-$ ..........$(5)$
The second ionization energy of $M$ could be calculated from the energy values associated with:

Amongst the following elements with their electronic configurations given below,which one has the highest ionization energy?

Which of the following has the lowest first ionisation potential?