00:01
In this question we're going to be looking at atomic orbitals, and we are looking at s orbitals and p orbitals.
00:13
So one factor about s orbitals is that the electron density is symmetrical and spherical.
00:23
So if we are to just draw this, say this is the x and y axis and we're going to have a dotted z -axis.
00:34
So what we are saying about the s orbitals, the electron density is spherical, spherical and it is symmetrical.
00:47
So what we are going to have is something like this to represent the electron density around s orbital.
00:55
But when we look at the p orbitals, here what we have here we've got lobes, two lobes that have got a node on the nucleus.
01:10
So when we draw this, say this is the y and x, y, x with a dotted z -exis.
01:24
What we're going to have is we have two lobes.
01:30
We've got two lobes with a node at the nucleus.
01:38
And another defining factor here is that they are not symmetrical.
01:45
As a result, if they are not symmetrical, it means we've got three pottes, three pots.
01:51
Serbon orientations or possibilities...