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Solution: Propose at least two different structures for a compound wit...

Question

Propose at least two different structures for a compound with six carbon atoms that exhibits the following features:

(b) Only one carbon atom is sp hybridized, and the remaining ve carbon atoms are all sp3 hybridized (remember that your compound can have elements other than carbon and hydrogen).

Video Transcript

Hey guys. So in this one we need to come up with at least two different compounds that have the structure of six carbons, right? And any other hetero atom that we'd like to use, right? As long as only one of our carbons is SP hybridized and all the other ones are sp3 hybridized, okay? So let's go ahead and take a look at this, what is an SP3 hybridized carbon have, we know that an sp3 hybridized carbon has four groups yes? I can't spell apparently, and SP hybridized carbon only has two groups, right? So now the easiest way to start off is to just draw six carbon chain, right? So there's a six for chain 1, 2, 3, 4, 5, 6 and if you take a look? Well, this one over here guys, how many groups does it have? well, it's got 3 hydrogens, we know that, and then it's got the directly attached to one carbon. So, 4 groups sp3 hybridized, this one in the middle how many carbons does it have attached? is got 2 carbons directly attached and it's got how many hydrogens? 2, so that's 2 plus 2 is 4, so that's an SP3 hybridized carbon an SP hybridized carbon, guys there's no way if we just go ahead and make, let me, this is not drawn correctly but just for illustration purposes and we've got a triple bond here between these two carbons, guys both of those only have two groups, right? This one's, this purple one over here and as green one over here, if you take a look, right? This purple on has this green carbon as a group and this blue carbon as a group and this green carbon has this purple carbon as a group and this yellow carbon as a group, right? So, does that really help us? not at all because we only we can only have one SP hybridized carbon, so what if we put it over here, our triple bond, same thing, right? We've got a hydrogen over here, right? So this carbon only has two groups on, this one in yellow it's got this purple one and this green one but now look at the green one, if we take a look, let me do it over here, and again this is not drawn properly, but guys if we take a look at this what's happening? Well, our green one only has the yellow and the blue, right? So it's also sp hybridized, okay? So that doesn't work but what if we do this, what if we instead of having our carbon there we have a nitrogen. Remember, that nitrogens like to have three bonds, right? So if we do this that kind of works, right? But let's go ahead and make sure we have the right number of carbons 1, 2, 3, 4, 5 ah, we're missing a carbon, right? Guys, actually no we're not, this carbon is right here, okay? The reason, we don't draw a triple bonds bent like this, okay? we draw the linear, okay? There's a very good reason for this, the theory would be that the two the 2p orbitals have to overlap, right? So you can't have one as way over here and another over here, for it to be, for it really work, you need two linear so, which you can have this something looks like this, that is the correct way to draw it, let's take a look at how many carbons we have 1, 2, 3, 4, 5, 6, right? This is the correct way. Notice that our triple bond is linear, over here it was bent if we drew it like this, right? That just doesn't work, so that carbon has to be somewhere in there, this is completely wrong structure though, this is the correct structure, so now that we know that you can use a triple bond and write a nitrile, what else can we do? well guys we can just have a five carbon chain and our nitrile coming off somewhere. So, we have a four carbon chain there, I'm sorry, five carbon chain there and now what if we just add 1, 2, 3, 4, 5, right? What if we just do this, we add our other carbon down here, triple bonded to our nitrogen, that works just as well, right? We've got 1, 2, 3, 4, 5, 6 carbons and our nitrogen and the reason that the nitrogen here, just to, the hybridization of the nitrogen here is also sp3, it's also SP, right? Because we've got the lone pair and this other carbon over here as Group, right? So we've only got two groups on that nitrogen, so it's also SP. Alright guys, let's move on.