00:01
So now we're going to work on problem 41 from chapter 5.
00:05
In this problem, we're asked to draw a loose structure for the acetate ion, including all resonant structures, and to indicate which atoms will have a formal charge.
00:18
So the acetate ion is usually written as ch3 -c -o -o -m minus.
00:27
So if we are to add up all these electrons here, we have eight from carbon atoms, 16 or sorry 12 from oxygen and three from hydrogen which makes 23 electrons but then we consider that we have one for the negative charge so we have 24 electrons total so as we start to draw these lewist structures here we're given a little bit of a clue about the structure based on how it's written so we have a carbon bound to three hydrogen atoms which is bound to the next carbon and then we have two oxygen atoms like this.
01:09
So we have our skeleton down based on the structure, the name that we're given.
01:16
So here we've included one, six bonds, so that's 12 electrons.
01:21
So we need to assign loan pairs to our outer elements first, outer atoms.
01:29
So we can put the additional 12 electrons around oxygen atoms.
01:33
However, what we see here is that carbon, the second carbon, is deficient of electrons.
01:37
It only has six.
01:39
So instead of having two electrons on one of these three loan pairs on one of the oxygen atoms, we're going to put a double bond here.
01:52
So now every atom has an octet...