00:01
So in this problem, we're as to calculate formal charge for six different atoms.
00:05
Let's start by defining what formal charge is.
00:08
The number of electrons, or e -minus, around a neutral atom, minus the number of lone pair electrons, minus half the bonding electrons.
00:22
And it's half because, of course, in a covalent bond, we are sharing electrons.
00:26
Let's start with this oxygen right here.
00:28
Oxygen is normally going to be six electrons.
00:34
We're going to subtract the lone pairs.
00:37
That's six in lone pairs minus one half of the bonding electrons, which is two.
00:43
So that gives us a negative one.
00:47
And in chemistry, we put the number first, followed by the sign.
00:51
If it's just a one, then you can just put the charge here.
00:55
Now, sulfur has the same bonding pattern as oxygen.
01:01
It has six valence electrons.
01:03
We're doing sulfur now.
01:06
Six minus the two lone pairs minus one half.
01:11
Six.
01:12
That's going to be positive one.
01:14
So this is a positively charged sulfur.
01:16
And finally, carbon.
01:17
Carbon likes to form four bonds, typically...