00:01
To draw the lewis structure for s -o -2f2, we first need to count the total number of valence electrons.
00:07
Sulfur has six, oxygen has six, and there are two of them.
00:10
Fluorine has seven, and there are two of them.
00:13
This gives us the total of 32 valence electrons.
00:17
If we bond each of the atoms to the central sulfur, and we give each of the atoms an octet with three lone pairs, we will have used up all 32 of the valence electrons and everything will have an octet.
00:32
Sulfur has an octet because it has four bonds.
00:36
All the other peripheral atoms have an octet with one bond and three electron groups.
00:41
However, when we assign formal charges to this structure where the octet rule is satisfied, fluorines have a zero formal charge, the oxygens have a minus one, and the sulfur has a plus two...