Drawing the Lewis Structure for NO3- (Nitrate Ion)
Transcript: This is the NO3- Lewis structure: the nitrate ion. Nitrogen has 5 valence electrons. Oxygen has 6, we have 3 Oxygens, and we need to add 1 for this valence electron up here. That gives us a total of 5 plus 18 plus 1: 24 valence electrons. Nitrogen is the least electronegative; we'll put that in the center, and we'll put the Oxygens--all three of them--on the outside. We'll put two valence electrons between the atoms to form chemical bonds. So we've used six; we'll go around the outside: 8, 10, and 24 valence electrons.
We can see that each of the Oxygens has 8 valence electrons, so its octet is fulfilled. But the Nitrogen only has 6 valence electrons. We can take 2 electrons from one of the Oxygens on the outside and move it between the Nitrogen and Oxygen to form a double bond. When we do that, this Oxygen right here still has 8 valence electrons, but the Nitrogen now has 8. So we have fulfilled the octets on all of the atoms in the Lewis structure for NO3-. At the same time, we've only used 24 valence electrons.
If you calculate the formal charges, you'll see that the Nitrogen has a +1 formal charge. These two Oxygens with the single bond have a -1, while the double bonded Oxygen has a formal charge of zero. If we add all these up, we'll find out that it equals -1, which makes a lot of sense because we have a negative on the NO3- ion. One more thing we need to do for the NO3- Lewis structure is put brackets around the structure to show that it is an ion and it has a negative charge.
So that's the Lewis structure for NO3-, the nitrate ion. This is Dr. B., and thanks for watching.