00:01
In order to look at the trend between a period going across from sodium to argon for the second ionization energy, first we need to consider what happens with the first ionization energy.
00:14
Ionization energy is the amount of energy required to remove an electron from the outermost energy level of an atom.
00:22
And as you go across the period, typically the trend that you see is that for the first ionization energy is that the amount of energy increases.
00:31
As you go from left to right.
00:40
And the reason for this is because the effective nuclear charge increases.
00:46
Effective nuclear charge is the attraction between the nucleus and the outermost electrons.
00:51
And as we go across the period, we have an increase in number of protons, which according to kulam's law, increases the effective nuclear charge.
00:59
So you would expect to see a similar trend for the second ionization energy.
01:03
And when we look at table 7 .5, we see for the second ionization energy a similar trend...
