00:01
To draw the lewis structure for each of these and predict vesper, we first need to count the total number of valence electrons.
00:09
Sulfur contains six valence electrons.
00:13
Chlorine contains seven, and there are two of them.
00:16
So this gives us a total of 20 electrons.
00:20
If we put sulfur in the middle and chlorine on each side, and then we provide each chlorine with three lone pairs, and the sulfur with two lone pairs, so it has an octet.
00:37
We would have used up all 20 of our valence electrons with four electron groups surrounding sulfur.
00:44
It's a tetrahedral electron group geometry, but with two of them being lone pairs, this is bent at approximately 109 .5, or more specifically, 107 degrees, this being the vesper geometry for the molecule, and it doesn't ask for hybridization.
01:09
Okay, so just vesper.
01:10
The next one is pi3.
01:14
Phosphorus has five.
01:16
Iodine has seven, and there are three of them.
01:20
So that gives us 26 valence electrons.
01:23
If we put phosphorus in the middle, and we put all three iodines around it, and we give each iodine an octet by adding three lone pairs, we would have used up 24 of the 26, so there's two more, as a lone pair for phosphorus, so phosphorus can have an octet.
01:46
With four electron groups, it's also tetrahedral with the electron group geometry, but with one of them being a lone pair, the molecular geometry, according to vesper, is trigonal parametal.
02:03
And then for the next one, we've got c -l -o, or i'm sorry, c -e -sper.
02:11
Cl2o.
02:12
Chlorine has seven.
02:14
There are two of them.
02:15
Oxygen has six.
02:18
So that gives us 20.
02:23
If we have 20 valence electrons, we're going to get something very similar to what we had up above with 20 valence electrons.
02:34
It needs to go back with chlorine.
02:57
We'll have oxygen in the middle.
03:00
The two chlorines on the side, each chlorine with an octet, three lone pairs, two lone pairs on oxygen...