00:01
So let's look at this chemistry problem about ionization energy.
00:04
And before it gets started, i recommend that you do the question yourself and come back to see if you go right or not.
00:10
So hopefully you've done the question.
00:12
So let's solve it together.
00:15
So we're given three elements in this case, which is nitrogen, oxygen, and fluorine.
00:19
And we want to know which one has the highest second ionization energy.
00:23
And to explain, let's define ionization energy first.
00:36
It is the energy required to...
00:43
Remove an electron from a gaseous element and it forms a gaseous ion right and then that means that the second ionization energy is basically the energy required to remove the second electron from gaseous ion to form a gaseous two plus ion right and as you we should identify the trends so as you go from left to right the periodic table the ionization energy increases and this is because a nuclear charge increases so there is a greater attraction between the nucleus and the outermost electron so there's less distance between the nucleus and the outer most electron thus more attraction so it requires more energy right to remove the outer most electron so that's why ionization energy increases so this is why according to the trend that we have just identified nitrogen should be the lowest and fluorine should be the highest.
02:03
But why is that not the case? to explain why, it would be helpful to look at the electrons and the animal shell of the elements.
02:11
And we can do that by writing out the electronic configuration of each of the elements...