00:01
This problem we're first going to look at n3 minus so each nitrogen will have five balance electrons and our minus charge means we add one more so we have 16 electrons so we have our nitrogen's here we can have double bonds on both sides of our central nitrogen and when we put in non -bonding electrons we can look at nitrogen having five valence electrons, two bonds, and four electrons here.
00:46
So we get negative one as the charge on both of these.
00:50
And then our central nitrogen has five valence electrons and four bonds.
00:56
So we have positive one.
01:00
Now we can also have where we have a triple bond on one side.
01:08
So for this nitrogen, we have five valence electrons, three bonds.
01:13
Bonds and two electrons, so we get zero.
01:17
Here we have five valence electrons, four bonds, and zero electrons, so we get positive one.
01:26
And here we have five valence electrons, one bond, and six electrons, so we get negative two.
01:39
And because we have smaller formal charges, this is going to be our more favored lewis structure.
01:48
And this is linear...