00:01
Okay, we need to give the lewis structure for hn, c.
00:06
Okay, so they're telling us the skeletal structure, right? we know that there's going to be an n in the middle, bond to c, and they bond to h.
00:18
The next thing i like to do is figure out how many electrons do we have to work with, right? hydrogen is in group one, gives us one electron.
00:28
Nitrogen, which is in group five, is going to give us five electrons.
00:34
And carbon.
00:37
Sorry, this is getting ahead of myself.
00:41
Nitrogen, which is atomic number seven, is going to bring, oh, sorry.
00:54
Nitrogen, which is in group five, is going to give us five valence electrons.
01:02
And carbon, which is in group four, is going to give us four valence electrons.
01:05
Okay, so we've got a total of ten electrons to work with.
01:10
We've used four of them, right? that each bond contains two.
01:13
We also know that hydrogen can only ever have a single bond and won't have any lone pairs.
01:18
So the remainder of the electrons will either have to be bonds between nitrogen and carbon or lone pairs on nitrogen and or carbon.
01:27
Something else we may know is that carbon being in group four always wants to have four bonds and no lone pairs.
01:36
That's pretty much the only way carbon can be satisfied without a formal charge.
01:40
Remember because formal charge is calculated as group number minus the number of bonds minus the number of electrons in loan pairs...
