00:01
Okay, so we're asked to draw a lewis structure for this compound, sf4cl minus, so it's an ion.
00:09
And specify the molecular geometry, and this is make sure to include all lone pair electrons and use solid -dashed wedge bonds if necessary.
00:18
All right.
00:19
So the first thing we do is figure out how many electrons we have here.
00:22
So we can start putting this together.
00:25
So sulfur has six.
00:27
There are four fluorine atoms.
00:29
Each one of those has seven plus another seven for the chlorine plus one for our negative charge that gives us a total of 42 electrons in this so we need to start drawing a structure for this and we're going to pick sulfur as our central atom because it will form at least two bonds where fluorine and chlorine only form one each and it also has a lower electronegativity so we'll put software in the middle.
01:00
Okay.
01:01
And then we're going to have to attach four fluorines and a chlorine to that.
01:12
That's five balance.
01:17
We're attaching to that.
01:18
So there's our four fluorines and chlorine here.
01:24
Okay.
01:25
We need to add our lone pairs of electrons.
01:28
I believe there's a different color here in front of it.
01:31
So if i count those up, now that's going to be eight around each one of these.
01:56
So 2468, 2468, 2468, 246, 8.
01:59
So 8 times 5 is 40.
02:01
So we have two more electrons...