00:01
Okay, so this problem asks us to use the localized electron model to describe the bonding in acetylene, which is c2h2.
00:09
And it says it exists as hcch, so it gives you the bones of the molecule.
00:16
The localized electron model is also referred to as drawing lewis structures, so if you're familiar with that.
00:21
Let's calculate our total number of electrons first.
00:24
So there's two carbon atoms and two hydrogen atoms in the formula from the subscripts.
00:28
And carbon normally has four valence electrons from being in group 14, and hydrogen normally has one valence electron from being in group 1.
00:38
So that's eight valence electrons to the carbons and two valence electrons to the hydrogens, which means ten valence electrons total.
00:45
Now when we draw our structure, hydrogen is supposed to follow the duet rule and have two electrons, which it does based on this bond, because bonds are really two electrons being shared.
00:55
So the hydrogen has two already, so the carbons are the ones that are not currently happy.
01:01
To make them happy but not have more than ten electrons, we're going to have to put a triple bond here.
01:06
That will give you eight electrons around each carbon...
