00:01
Okay, so here we want to draw the resonant structures for hc &o.
00:04
So here we want to go ahead and just draw it, how, draw the skeleton, how it's arranged in the formula, and then we can go ahead and see how many valence electrons we have to work with.
00:14
So for carbon, it has four valence electrons, nitrogen has five, oxygen has six, and hydrogen has one.
00:22
So overall, we have 16 electrons to work with.
00:28
Now, because we've already done, use three bonds, that's using ups, six electrons, so we'll go ahead and take six away, which leaves us with 10 to work with.
00:37
So what we know is we know that oxygen typically makes two bonds, nitrogen typically makes three bonds, and carbon typically makes four bonds.
00:45
So what we can do is we can go ahead and add in bonds for these components, starting with carbon.
00:53
So if we put a triple bond here, carbon now has four bonds, but nitrogen also has four bonds.
00:59
So carbon is happy, but nitrogen is probably going to have a formal charge.
01:03
Because we've added in two bonds, we'll take away four electrons, meaning we have six left to work with.
01:11
Because oxygen typically wants two bonds, but nitrogen has too many bonds already, or it has four bonds already, we can't add any more to it, which means we're going to need to satisfy oxygen with just lone pairs instead of another bond.
01:24
So we'll add in three lone pairs for oxygen, which uses up the rest of our electrons.
01:29
So now we have a structure where all the octets are satisfied, but we're going to have some formal charge.
01:37
So carbon typically wants four bonds, so it's not going to have any formal charge.
01:41
But we'll have to calculate the formal charge for nitrogen and oxygen.
01:45
So what we do is we take the valence electrons minus the number of bonds, minus the number of lone electrons...