00:01
To determine the expected hybridization around the central atom, we'll draw the lewis structures for the ions or molecules that we are considering.
00:07
For this one, we have selenium trioxide.
00:11
After counting up the number of valence electrons, we find out that we have to double bond to selenium in order to get a complete octet on selenium with one of the oxygens.
00:22
There would be two more resonant structures, of course, where the double bond could be here, or the double bond could be here.
00:27
So the hybridization then with three electron groups, one of a double bond and two of them single bonds would be sp2 hybridized.
00:37
Then we have selenium dioxide.
00:40
And with the number of valets electrons available, we need to share electrons from one of the oxygens as a double bond.
00:49
So we could put a double bond on the right as shown or a double bond on the left.
00:54
We still need a lone pair on selenium, which we have in order for selenium to have an octet.
01:01
That then gives us three electron groups surrounding selenium, one a double bond, one a lone pair, one a single bond.
01:07
So three electron groups is sp2 hybridized.
01:12
Then we look at phosphorus trichloride.
01:15
And with phosphorus trichloride, there are 26 valence electrons that are available after putting an octet around all...
