IE is the amount of energy required to remove the outermost electron from an atom to create a positive ion. Electrons are always removed from an atom/ion one at a time and so most atoms (all except hydrogen) will have more than 1 ionization energy. Each successive ionization energy for a given element represents the removal of a subsequent electron. The table below contains the first 4 ionization energies of magnesium. Our goal is to write the IE equations for all four IE values, but before we do that, let's make sense of the values in the table. IE: 896 kJ/mol IE2 1752 kJ/mol IE4 IE3 14,807 k]/mol 17,948 kJ/mol Part 1. Discuss the following questions with your group. 1. It is often said that all of chemistry is governed by electrostatic interactions. What do you think holds the electrons of Mg to its nucleus? 2. Why do you think the ionization energy for Mg increases as you go from Ii to l4? 3. Why do you think there is such a large difference between the 2nd and 3rd ionization energies of Mg?