00:01
First off, we are looking at s2.
00:04
Oh, let's get to the writer.
00:06
There we go.
00:08
S2f10.
00:09
Now, if you don't intuitively know how these are going to connect, it's okay.
00:13
Some of these get so complicated, you do kind of have to look it up to get some hints.
00:17
And for this one, since sulfur is the least electronegative.
00:21
Okay, remember, electronegativity increases as you move up into the right, maxing out at fluorine.
00:29
Okay.
00:29
So in this case, flooring is the most electric negative bottom.
00:34
Okay, that means we're going to put sulfurs in the middle, and we're actually going to connect them.
00:38
Okay, so we're going to have two sulfurs in the middle, and then we're going to distribute the fluorines around those two.
00:45
So five each.
00:47
Two, three, five.
00:52
We've got to put another one in.
00:53
We'll go right there.
00:55
One, two, three, four, five.
00:58
All these are going to be fluorines.
01:07
Floring, flooring, flooring, flooring, flooring.
01:09
And fluorine.
01:11
Okay, now we do need to know our total valence electrons so we know when to stop adding dots, right? that's why i have this periodic table app shows you your valence electrons.
01:21
So sulfur comes in with six valence electrons.
01:28
Now there's two of those, so it would be two times six for sulfur.
01:34
Two times six.
01:36
And then the fluorines have seven valence.
01:42
There we go.
01:43
So this is going to be 10 times 7.
01:47
Oh, goodness.
01:48
This is a lot of electrons.
01:49
We've got 82.
01:52
Now, so far, each bond has two electrons, and we have drawn 11 bonds.
01:59
Yes, 11.
02:01
So 11 times 2 is 22.
02:06
82 minus 22 drops us down to 60 electrons to go.
02:11
We'll start with our outer atoms.
02:13
Each of those fluorings currently has two electrons.
02:15
It needs eight.
02:16
So each flooring needs six more.
02:35
Okay, six times 10 gives us 60.
02:40
So we are out of valence electrons.
02:42
Double check that your sulfers are happy.
02:44
They're more than happy.
02:45
They actually have broken their octets.
02:48
So they actually have one, two, three, four, five, six, twelve electrons each.
02:53
So we are more than done.
02:55
Okay.
02:56
Now, it looks like we also care about, let's see.
03:07
Nope, that's it.
03:08
We're good, actually.
03:09
Everybody's happy.
03:10
Okay.
03:11
Then let's move on to the second one.
03:16
For this one, we are doing f -x -e and this is a piece of work.
03:24
S -o -2f and 2.
03:28
All right, this thing is a beast.
03:31
That's okay.
03:32
That's why we're here.
03:33
We're going to do it together.
03:35
Okay.
03:36
So first thing to look at is who is going to be your central atom for? this.
03:40
Now, obviously, there is a lot happening.
03:43
But first off, central atom.
03:47
Look for your least electronegative.
03:49
We've got, remember, that's closer to fluorine.
03:52
So we've got fluorine.
03:53
We've got a xenon all the way down here.
03:56
Okay.
03:57
We've got nitrogen.
03:59
We've got sulfurs.
04:01
We have oxygens and we have fluorines.
04:04
Now, the reason they put the so2f in parentheses is because that bonds together as a group.
04:10
So those, so the parentheses part is going to stay as a chunk.
04:14
So we're not going to consider that for a central atom.
04:18
So that leaves nitrogen.
04:23
Up into the right.
04:24
So nitrogen is your least electronegative atom there.
04:28
So we're going to put nitrogen in the middle.
04:32
Now, the way you arrange this around it, there's a little bit of give and take as to how to do this.
04:39
But there's going to be two groups of the so2f.
04:46
Now, those are sulfers that have two oxygens and a fluorine attached.
04:55
Okay.
04:56
And we're going to put one on either side because there's two of those.
04:59
So s, and you can rearrange the oxygens and fluorines however you want, as long as everybody's connected to that sulfur.
05:07
Okay.
05:08
Next, you have the xenon and the flooring.
05:11
Okay.
05:12
Now, there are a couple ways this could have been done.
05:15
One way would have put to put a xenon up here and a fluorine down here.
05:20
That is not likely just because nitrogen, if given the option, would rather have three bonds instead of four...