b. Draw the resonance forms for ozone (bonded OOO )
c. Sulfur dio...

Question

b. Draw the resonance forms for ozone (bonded OOO ) c. Sulfur dioxide has one more resonance form than ozone. Explain why this structure is not possible for ozone.

Accepted Answer

Hey everyone. Let's solve this problem. It reads compare the resonance forms of try sulfur S. Three and ozone 03. There is an additional structure possible for try sulfur which was not present with ozone. Explain the reason behind this additional resonance form for try sulfur. So first let's draw the structure for ozone. And then when we get to try sulfur, we'll talk about the differences between sulfur and oxygen and see why we can have that additional resonance structure. So first, when you're drawing a resonance structure or lewis dot structure, you want to count the total number of electrons that should be on your structure. How do we do that? Well, you remember we look at the number of valence electrons from the periodic table. So oxygen Can have six valence electrons And there are three oxygen's in ozone. So that gives me a total of 18 valence electrons. Okay, so my structure should have 18 electrons. Let's draw three oxygen atoms connected. Now I know this oxygen can have two lone pairs, 1234, there's one adam touch or one electron touching it in this bond. So if I add a double bond that gives me 1/6 electron touching it right there. So this oxygen is very happy. It has six electrons touching it. It has eight total valence electrons to four from the double bond and four from the lone pairs. So let's look at the center oxygen, let's see 123 electrons touching it. If I add a lone pair, that's five. Could I add a double bond and make it six with a total of 10 valence electrons on the center oxygen. No, because that violates the octet rule. Right, so let's just leave that oxygen with five and give it a plus charge. And now remember we said we want 18 valence electrons. So that means we have six left 123456. Well, this oxygen only has seven total but it has seven. Or sorry, it has seven electrons touching that oxygen. So that gives it a negative formal charge. So that is the first structure. Now I can basically swap that double bond to the other side. The center oxygen keeps up plus one charge. And now the left side, the oxygen on the left side will have that negative charge. Alright, so now let's look at sulfur. The mysterious sulfur or I should say try sulfur. Right, so sulfur has how many valence electrons? It also has six valence electrons because it's in the same group as oxygen. And there are also three sulfur atoms. So we should also have 18 valence electrons. Well, because the electron number is the same and there are also three cell furs. I will have these same two resonance structures for sulfur. So let's draw those positive charge in the center sulfur negative charge on the right hand, sulfur and double bond between the left and center sulfur. Now I have the double bond on the right hand side, sulfur positive charge still on the center and negative charge on the left hand sulfur. Well, what did I say in when we were drawing ozone that I can't do because it would violate octet rule. I said I couldn't draw a double bond on both sides, right? Because again there's a lone pair here on that center sulfur. And that would give me 2468, 10 sharing valence electrons. And that violates octet rule. Right? Well, like the problem said, sulfur has an exception. Why is that? Well, let's look at the electron orbital configuration of sulfur. Just the valence show. So it goes to the three end sub show And we said it has six electrons right? 123456. So that means I have two lone pairs, right? And then the ability to make two two bonds. Okay, so that would give me eight electrons. Right? That's normal. Just like oxygen. But what's different is sulfur has this three D shell right here. And these electrons can Increase their energy and jump to that three D orbital. And it would look like this. So the paired electrons in the three p. Show. And this could also happen with three S. But in this case it's three p. So that electron that was here in the first little shell will jump up to the D orbital giving me one lone pair. And now the opportunity to make four bonds. And because there's two electrons in every bond and a lone pair. This gives me the opportunity to have 10 valence electrons. And this is called hyper valence, see which we do not see in oxygen. Okay, so that's why sulfur can have this expanded octet and it can have 2468, 10 electrons here on that center, sulfur. And that gives us the resonance structures for ozone and try sulfur. I hope this video is helpful, and thanks for watching.

b. Draw the resonance forms for ozone (bonded OOO ) c. Sulfur dioxide has one more resonance form than ozone. Explain why this structure is not possible for ozone.

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