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Solution: What is the hybridization of each carbon in CH 3CH=CHC≡CH?  ...

Question

What is the hybridization of each carbon in CH 3CH=CHC≡CH?  What are the CCC bond angles? 

 

Video Transcript

Alright everyone. So, for this molecule we're going to be doing a couple things, one being to identify the hybridization of each atom here, so let's look at our five carbons, we have 1, 2, 3, 4 and 5 and for a better representation we can actually draw this out, what we're going to do that is we're going to represent a CH3 group right here we're now going to indicate that you have a carbon double bonded to another carbon, from there we have one hydrogen coming off and another hydrogen coming off here and then we're going to draw a line down that has a carbon triple bonded to a CH, okay? so let's take a look, let's start with this carbon right here, it's got bond to three hydrogens and another carbon, so we're going to say that's, what? got better, it's going to be SP3 because this carbons is connected to 3 other atoms or four other atoms 3 hydrogens and one carbon, what about this carbon? Well, it's connected to one carbon, it's double bonded to another carbon and it's connected to one hydrogen, so that means SP2 if it's connected to 3 things. Now, let's take over to the next carbon, here similarly to the last one's going to be SP2, let's take a look at this carbon and this carbon, what do you think their hybridization is going to be? we're going to say that they're both going to be the same hybridization because they're both connected to one carbon at least the bottom was connected to one carbon and one hydrogen, and the top carbon is connected to one carbon and another carbon, so remember that this one's SP and this one's SP hybridized, okay? Now, we need to actually calculate the bond angles, so what we're going to do that is we're going to be taking a look at this bond right here, we're going to take a look at this CC bond and we're going to take a look at the CC bond, okay? For the bottom one notice we have a triple bond, both of these atoms are going to be SP, so we're going to say that this is going to have a linear geometry in be a 180 degrees, okay? Now, if we take a look at the other carbons. Notice that this one right here and this one right here are both sp2 hybridized and what that means everyone has a bond angle, between this carbon and this carbon and this carbon and this carbon we expect that to be trigonal planar and that means it's 120 degrees, similarly, let's write that over here, similarly, let's look at the other bond. Now, we're going to be highlighting this bond and this bond and notice that what you'll see at the bottom is only another 120 degree angle because that carbon is sp2 hybridized, okay? So we're going to say, this is going to be 120 degrees as well, okay? So, just remember that trigonal planar means is going to be 120 degrees and linear such as a triple bond will be a 180 degrees, okay? So I hope this makes sense on how we only did the hybridization, right? SP, SP2 and sp3 but also we need to calculate the CCC bond angles, alright? So when you draw your structure it should be represented as one line here a double bond another line and then we have a triple bond, so that's how we got 120, another 120 and finally 180 for a triple one, okay? So, let me know if you have any questions.

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