00:02
To answer this question we need to start by drawing the lewis structure for h bonded to o to c to n.
00:12
So let's go ahead and do that.
00:13
We have hydrogen, we have oxygen, we have carbon, and nitrogen.
00:21
Okay, hydrogen we know has just one valence electron.
00:24
Carbon has six, i'm sorry, oxygen rather has six.
00:28
It has two lone pairs and then two non -bonded electrons.
00:33
Carbon we know has four unbonded electrons.
00:37
So one is going to be used to form the bond to the oxygen.
00:42
The other three are going to partake in a triple bond with nitrogen.
00:49
Because nitrogen has five valence electrons, three unbonded, and one lone pair.
00:56
Alright, so this would be our lewis structure.
00:58
We are ready to answer our questions.
01:01
First thing we want to know is the o to c to n bond angle.
01:05
So we want to know this angle here.
01:10
Well, to answer that we need to know the geometry around the carbon.
01:15
Carbon has two atoms bonded to it and zero lone pairs.
01:20
So anytime we just have two electron domains, which is what we have here, it is going to be linear.
01:26
So it is linear about the carbon, which means that this would be a 180 degree bond angle.
01:34
So our first answer is 180 degrees.
01:37
To answer our next question, we are trying to identify the type of bonds.
01:46
Sigma bonds are end to end overlap.
01:50
And all single bonds are sigma bonds.
01:56
And the first bond in a multiple bond is a sigma bond.
02:06
So a multiple bond, i mean a double or a triple.
02:09
Pi bonds on the other hand are those remaining bonds.
02:17
They are side to side overlaps of the orbitals.
02:21
And they are the remaining bonds in a multiple bond.
02:24
So a double bond would have one pi bond.
02:32
And a triple bond would have two pi bonds...