00:01
To draw the lewis structure, we first need to count the total number of valence electrons.
00:05
We have c2, hbr.
00:10
Carbon has four valence electrons.
00:13
There are two of them.
00:14
Hydrogen has one, and bromine has seven.
00:19
So this gives us a total of 16 valence electrons.
00:25
Carbon is typically in the middle, so we're going to have to have carbon bonded to carbon.
00:31
But in order to make this work, we're going to have to have carbon.
00:35
Have to bond them in a linear chain.
00:43
Then this would use up one, i'm sorry, two, four, six, two electrons per bond.
00:49
So we've got 10 left.
00:52
If we give bromine an octet with three lone pairs, would have four left.
01:02
And if we put those four, say, on one carbon as lone pairs, then we'll find out that this carbon does not have an octet.
01:12
Hydrogen doesn't have an octet, but it only needs two and it has two.
01:17
So that means we're going to have to share.
01:19
And these lone pairs are going to have to become bonding pairs, forming a triple bond between the two carbons.
01:29
Now we have an octet...