00:01
So for this question, you're asked to find which elements are diamagnetic.
00:06
So remember, if an element is diamagnetic, that it means that all of its electrons are paired.
00:26
And then conversely, we have paramagnetic, and paramagnetic is when there are unpaired electrons.
00:35
But we are just focusing to determine if they're diamagnetic.
00:38
Bi -magnetic.
00:39
So in order to figure out if its electrons are paired or unpaired, we have to find its electron configuration.
00:50
So first let's start with francium, which you look at our periodic table.
00:56
It's over here.
00:57
So its electron configuration would be, let's use the noble gas configuration.
01:03
So we have radon and then 7s1.
01:09
So we know in the noble gas configuration, we have radon.
01:11
So we know in gas core, all of the electrons are paired.
01:15
So we're just worried about the valence electrons.
01:18
So the 7s1.
01:20
So we only have one electron in the s block.
01:23
So we have one orbital for s.
01:27
We got one electron.
01:28
It is unpaired.
01:30
So francium is paramagnetic.
01:33
So that is not diamagnetic because that has an unpaired electron.
01:37
Next we'll go to zirconium, which is a ion and this 2 plus means that we lose two electrons.
01:47
So first let's find the normal configuration for zirconium, which would be krypton, and then 5s2 for d2.
02:02
Now the 2 plus means that we lose two electrons and we're going to lose the electrons from the shell with the highest n number, a principal quantum number, which is five.
02:17
So we're going to lose those two electrons.
02:21
The iron.
02:22
So zirconium 2 plus would be krypton 42.
02:25
So again, noble gas core, all those electrons are paired...