00:01
Ok, so we're drawing some lewis structures here.
00:04
So first one, we have h, n, n, h.
00:08
And we're going to need a double bond here, two lone pairs here.
00:11
That'll give you your total of 14 valence electrons that you want.
00:16
Next one, you have h, o, cl, o.
00:22
Let's see here.
00:23
We could do, let's see, we're going to need 7, 12, so 20 electrons total.
00:29
If we just work on getting them up to the proper number, let's see how that looks.
00:35
So we've got 2, 4, 6, 8, 10, 12, 14, 16, 18, 20.
00:39
So i guess that's what we're working with.
00:41
It would be something like that.
00:44
We could technically break the octet rule on the chlorine to make its formal charge a little bit better.
00:49
So let's try that, actually.
00:52
So if i got rid of that, put a double bond here instead, then we'd still have 8 on the oxygen.
00:58
And the chlorine's breaking the octet rule, but it's actually making its formal charge better.
01:03
So that would be the best structure for b.
01:07
C says h, o, o, h.
01:11
I want to put a double bond here, i assume.
01:15
No, no we won't.
01:17
No, let's not do that.
01:19
So we'll put lone pair, lone pair, lone pair, lone pair.
01:22
Let's check our total.
01:23
We should have 14 this time, so 2, 4, 6, 8, 10, 12, 14.
01:27
Yep, there you go.
01:27
And everybody's formal charge is 0.
01:32
D, you've got, it looks like, se, o, oh, 2.
01:40
Your formatting's a little odd.
01:41
It says two of the seo bond lengths are 189, and one of the seo bond lengths is 170.
01:48
So the 170 one would be a shorter one.
01:50
That would be a double bond...