Question

6.24 This figure represents the successive ionization energy of an atom in the third period of the periodic table. Which atom is this most likely to be? 6 12,000 10,000 8000 Energy (kJ/mol) 6000 4000 2000 Ej1 E2 E3 E;4

explain and write clear please??

Answer 1

The amount of energy needed to remove the most loosely bound ekectron from the valence shell is called ionization energy.

The figure represents the Magnesium element which belongs to group third and has atomic number 12.

The electronic configuration of magnesium is 1s2 2s2 2p6 3s2. The first electron removals needs less energy because it is loosely bound to the atom. Then we have 3s1 electron which is closer to nucleus hence requires more energy. Once both of the electron is removed the configuration becomes an inert gas configuration. Therefore the 3rd and then consequently 4rth ionization energy is too high.