00:01
Okay, so if we want to draw the orbital diagrams for elements, remember how electrons fill in our atoms.
00:10
First, the 1s is filled followed by the 2s, the 2p, the 3s, the 3p, the 4s, etc, etc.
00:21
But we're only going to go up to 4s in these examples.
00:24
And remember that the s orbitals can hold two electrons, and the p orbitals can hold.
00:30
Six electrons.
00:34
So as we start out, if we start out with sulfur, which has 16 electrons, we're going to go ahead and fill up the orbitals.
00:47
We'll start with our 1s and our 2s, r2p, 3s, and 3p.
00:57
And remember that each orbital, each of these rooms here can hold two electrons, they're really suborbital.
01:05
So we have one, two, three, four electrons.
01:09
Remember that the electrons go in in opposite spin, so we show them in opposite directions.
01:14
Remember, hun's rule says that we fill electrons in each of the suborbital's first before we fill them in.
01:24
And then we have our s.
01:26
And now here for the p, we have to get to 16 electrons.
01:30
And so far, we have 12.
01:33
So we have to add four more.
01:34
So we'll add by huns rule, one, two, three, and then the fourth one.
01:40
Those other two will be left empty.
01:45
If we go and do calcium, this is going to require even more orbitals.
01:50
It's number 20 on the periodic table.
01:53
So we're going to have to account for 20 electrons...