Which one of the following has the lowest ionization energy?

For elements $B$,$C$,$N$,$Li$,$Be$,$O$ and $F$,the correct order of first ionization enthalpy is:

The first ionisation potential $(IP)$ of the elements $Na$,$Mg$,$Si$,$P$,$Cl$ and $Ar$ are $5.14$,$7.65$,$8.15$,$10.49$,$12.97$ and $15.76 \ eV$,respectively. The $IP$ (in $eV$) of $K$ is closest to

Which of the following electronic configurations represents the atom with the lowest first ionization enthalpy?

Consider the following ionization enthalpies of two elements $A$ and $B$.

Element	Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$
$A$	$899, 1757, 14847$
$B$	$737, 1450, 7731$

Which of the following statements is correct?

Which of the following electronic configurations represents a sudden large gap between the values of second and third ionisation energies of an element?