00:01
Hello students let's begin with this question.
00:02
This question is based upon the formal charge.
00:06
So the formula used to find out the formal charge is equals to the valence electrons minus the non -bonded electrons then here will be this will be minus the half of the bonded electrons.
00:27
So here we have to find out that which nitrogen has the formal charge is equals to minus 3.
00:40
So here the first one is n2.
00:44
So here if we see this is the structure of the n2.
00:49
So if we calculate its formal charge this is equals to nitrogen have 5 valence electrons minus the non -bonded electrons are 2 minus the bonded electrons are 6 by 2.
01:00
So it will have 5 minus 5.
01:03
So this will have formal charge is equals to 0.
01:05
So this is not the option.
01:07
Now the second one is the no.
01:09
So its structure is so nitrogen have the 5 valence electrons and oxygen will have the 6 valence electrons.
01:18
So now its formal charge is equals to nitrogen has 5 valence electron minus the non -bonded electrons are 3 minus bonded are 4 divided by 2.
01:31
So this will have a 0 formal charge.
01:34
So this is also not the option...