 Okay, so I've already got a Vesper theory video associated with acetylene, so you can go ahead and watch that But remember, this time we're actually going to be hybridizing the orbitals of one of those two carbon atoms Okay, so let's draw acetylene out just to remind ourselves what it looks like Okay, so can you guys tell me what does it look like? It's H with a bond to C with a triple bond Very good to a C then Very good guys, okay, so that's great So we're going to be looking at the hybridization of that carbon there So when we're doing these hybridization problems, the first thing we're going to do is write the valence shell of the actual unhybridized carbon atom Okay, so how do we do that? Remember, we're going to draw an electron diagram, so what's going to be down here? What are we going to put? Well, just the valence shell Two of us Okay, so I know we were doing the whole thing before, but once you get to the bigger atoms, then it kind of starts being cumbersome to do all the lower levels Because only the valence shell participates in the chemical reactions So the bottom, what did we say? Two S And the next is going to be two P And how many orbitals there? Three One, two, three So we look at this and we look at this, we look up here, okay, look up at the bigger table And let's fill this up by all of our filling rules, okay So what is it going to look like here? How many electrons? Two Two One up, one down And here, how many? Two One One Here One Here None Okay, so that's the carbon unhybridized, right? What are we going to do? We're going to stick it in the blender, right, and hybridize it Are you okay with that? So we're looking at that carbon How many sigma bonds is that carbon making? Two Two, okay So how many orbitals need to be hybridized? Two We need, yeah, we only need two, okay So which one definitely has to go? The S and one of the P's, right? So I'm just going to do that, box those guys in So those are the two that get thrown in the blender and hybridized, okay So if we put two in, how many are we getting now? Two Two And what is the name of those two? That's P Why? Because I used one S and one P Does that answer your question now? Okay, good We're going to still go through the rest of this, though What happened to these other orbitals? They're on the top, okay So, and they're still what? They're P's, right? Yeah, they're P orbitals, okay So now we're going to take these electrons here and throw them in to these orbitals, okay So how many electrons here? One One, yeah, for each orbital Here, one, why? Because they're going to make sigma bonds We know that, right, okay And what about here? One One And do we have any more? How many do we have? One, two, three, four, right How many do we have over here? One, two, three, four, right Okay, so let's go back and draw that Lewis structure again Doing how we do with the Fischlkaros, okay Just to remind ourselves So, remember, these are the sigma bond forming, right And these are the pi bond form, okay These ones here So, okay, so we're focusing on this carbon here But we can do both of them So everybody's okay with that formation, right And of course I'll bet you everybody's okay with that one too, right So let's go ahead and life those away And draw actual covalent bonds in between there Like that, right How many more bonds does this carbon want to make? Two Two more Can it make two more with this one here? Yes Yeah, okay So what you'll find is these two electrons Are this electron and this electron here And the p orbitals, okay So the electron that was here previous And the electron that was here previous Are these two electrons here, okay So when we do that, like that What do we make in between those two carbon atoms? A Pi Well, how many pi bonds? Two Two So pi bonds come from these p orbitals there, okay So if you've got two empty ones Or half empty ones then you're going to make a triple bond You've only got the one half empty one Like we did with the sp2 structure It's just going to make the double bond, okay So what would be the bond angle here? 180 180 If this is, what's the hybridization of that carbon again? Sp If this is sp, that's 180 Okay Is everybody okay with hybridization? Okay, this is a more difficult problem So if you're cool with this Then you should be good with everything else Is there anything else anybody wants me to ask Or any questions on this one in particular? You're cool with hybridization now? Okay, go ahead Just a quick question Two sigma bonds You only pick two of the lowest levels, right? Yeah, you take the lowest level first Within the valence shell, okay And all of those electrons have to be pushed over Into the new orbitals, okay Any other questions? That's a good question Okay, wonderful