Ionization Energy as a Periodic Property

Let's see how ionization energy is a periodic property. Just as was the case for the periodic trend of atomic radii, the logic behind the periodic trends for ionization energy can be understood by understanding the effective nuclear charge. Moving from left to right across a period in the , the atomic number, and therefore nuclear charge, of each increases. However, moving down a group in the , the increase in atomic number is "shielded" by the increasing number of electron shells surrounding the nucleus, and consequently, the effective nuclear charge decreases.

In general, the greater the effective nuclear charge of an atom, the more closely the electrons are held, and consequently, the greater the ionization energy. This logic explains the following periodic trends for ionization energy:

Moving left to right across a period, the ionization energy increases (as the nuclear charge increases)

Moving down a group from top to bottom, the ionization energy decreases (as the effective nuclear charge decreases due to the shielding effect of the electrons)

(Note: There are a few minor exceptions to these trends, but it is most important now for you to understand these general trends in ionization energy.)

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