Video Solution: The connectivity of carbon oxysulfide is OCS. (a) Writ...

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The connectivity of carbon oxysulfide is OCS.

(a) Write a Lewis structure for carbon oxysulfide that satisfies the octet rule. 

Video Transcript

So let's say we need come up with the lewis structure for carbon oxysulfoxide, okay? It's connected like this, okay? It's O C S. Now, let's go ahead and fill things in using our bonding preferences, okay? we're not going to do this as Gen chem way, we're going to do it the way that makes sense to me and hopefully will make a lot more sense to you intuitively, so we've got oxygen, right? We've got our carbon and we got our sulfur, guys our central atom here is our carbon, why? because it's the least electronegative atom, right? Let's go ahead and give ourselves our chem 7, which you guys will probably become very familiar with as the course goes on, okay? So we've got carbon, nitrogen, oxygen, fluorine, bromine and iodine, okay? These are our main elements that we're going to be dealing with in orgo, we've also got, here we got sulfur, which is right under here, okay? And what do we know about electronegativity? we know that electronegativity increases as we move up and as we move to the right, okay? And that will become important in the next part of this question. Guys, since our carbon is in the middle we know that it probably wants to have its bonding preference, right? What's that going to be? we know it's going to have four bonds, okay? but, where? Well, here's where another point of knowing our bond preferences comes into play, right? Oxygen likes to have two bonds and two lone pairs, right? And guys, so does sulfur, most of the time because it's directly under oxygen, you're going to see a lot and sulfur can expand its octet, especially when it's convenient, right? But here we've got our double bond to oxygen and double bond to carbon. Now, what do we expect to have? we expect to have our oxygen with two lone pairs and same thing for our sulfur, okay? Now, everything has its octet completed. So, my next question is what do you expect the geometry of this molecule to be? do you expect it to be bent, like what do you, what do you think it's going to be? bent, something else, linear. Guys, it turns out that it's actually going to be linear why do you think that might be? Well, notice something, we've got accumulated double bond, right? We've got a carbon that's got double bonds on both sides, so it's got to have PI orbitals, right? It's going to have P orbitals to form a PI bond on one side but once it does that it needs to have the PI orbital, the P orbitals place the pi bond behind it as well, right? So we need to have it on both sides lined up, so it's forced into a linear geometry, okay? And do we expect there to be a dipole in this molecule? we do, right? We actually expect because of our electronegativity, we expect 2 dipoles but one net dipole, okay? we expect there to be a dipole pulling away towards the oxygen and pulling away from the carbon toward the oxygen and we expect from the carbon to the sulfur, but what's more or less than negative here, oxygen or sulphur? definitely oxygen, right? So, our two our net dipole is going to be pulling toward our oxygen, okay? Alright guys, let me know if you have any questions I hope that helps, if not, let's move on. There are no questions.