00:01
Out here and the first thing we need to fill out is does this have polar bonds? yes, this has a c -h which is polar and c -c -l which is polar.
00:11
Yes, this has c double bond -o and that's polar and yes h -n is polar.
00:19
Do they have loan pairs on the central? no, no and yes, as you can see the loan pairs on the central right there.
00:30
If there are polar bonds are they symmetric and yes and no.
00:42
So this one is polar.
00:46
This is non -polar and this is polar.
00:53
That's everything we're supposed to fill for the first table.
00:56
For a second table, we're asked to write the formula for methane, then from formaldehyde, aldehyde, and then for xenon tetrafluoride.
01:24
And let's do these.
01:33
Okay, okay, hang on here.
01:49
So let's get our formaldehyde lewis structure.
01:54
Will be c .h.
02:05
And then i think it'll be double band.
02:08
Oh, i think this is going to be my lewis structure of this.
02:17
Yes.
02:17
And then my xenon, tetra, lewis structure.
02:32
I think that's going to be a square planer.
02:37
Yes.
02:38
So this will be, like the general idea there.
03:05
Okay, let's get back to our question and see what i'm supposed to be doing.
03:09
Okay, the structure we're done with.
03:21
Then polar bonds, which, just like the last, this will be c -h, this will be c -h and o double bond c, and this will be x -e -f.
03:42
Does the molecule have lone pairs? lone electron pairs on the central.
03:52
Adam, no, no, and yes.
03:58
If there are polar bonds or lone pairs, are they symmetric? if there are polar bonds, are they symmetric? yes...