What explains the change in ionization energy that occurs between removing the first and second electrons from an atom

Options are as follow,

A. The ionization energy decreases because the ratio of the protons to electrons increases.
B. The ionization energy increases because the ratio of the protons to electrons increases.
C. The ionization energy decreases because the ratio of the protons to electrons decreases.
D. The ionization energy increases because the ratio of the protons to electrons decreases.


            Option-B (The ionization energy increases because the ratio of the protons to electrons increases).

Explanation:
                  Ionization energy is the amount of energy required to remove one electron from the valence shell of an atom.
                  Also, first IE is energy required for removing electron from neutral atom, 2nd IE is energy required for is for removing electron from a mono positive atom and so on.
                  Example:
                                  1st IE of Na is 495.8 kJ/mol

                                   2nd IE of Na is 4562.4 kJ/mol

Second ionization energy is greater because after the removal of first electron the ratio of protons to electrons increases, resulting in more nuclear effect. Also, the second IE is greater because the Na⁺ having noble gas configuration is a stable state, hence more energy is required to knock out electron from it.

All the elements are arranged by melting points on the periodic table. in row they go from metals to gasses. in the row from sodium to argon, sodium is more reactive than the one on its right, magnesium.