The correct trend in the first ionization enthalpies of the elements in the $3^{rd}$ period of periodic table is:

The five successive ionization enthalpies of an element are $800, 2427, 3658, 25024$ and $32824 \ kJ \ mol^{-1}$. The number of valence electrons in the element is

An atom with high electronegativity has

The values of $\Delta _iH_1, \Delta _iH_2, \Delta _iH_3$,and $\Delta _iH_4$ for an atom are $7.5 \ eV, 25.6 \ eV, 48.6 \ eV$,and $170.6 \ eV$ respectively. Determine the electronic configuration of the atom.

The successive ionization enthalpy values for an unknown element are $\Delta_i H_1 = 899 \ kJ/mol$,$\Delta_i H_2 = 1757 \ kJ/mol$,$\Delta_i H_3 = 14847 \ kJ/mol$,and $\Delta_i H_4 = 17948 \ kJ/mol$. To which group of the periodic table does this element belong?

Which of the following atoms has the highest first ionization energy?