 So, let's do that same sort of analysis with this hydrogen cyanide. So we'll see how the central carbon rehydrates, okay, to make the molecular orbital. So carbon, right, is what we're looking at, and we got to look up at the periodic table and find where carbon is, and draw its molecular orbital diagram before it's failed. So when we do that, we notice it's got a 2s, and it's 3, 2 p's, and it's got 1, 4. So what's going to happen here? So what do you know what the hybridization of this is just from bond angle? Do you remember what that is? It's sp. It's sp, right? So knowing that should kind of promote you to get the right answer here, okay? So it's sp, right? That carbon is sp-hybridized. So it's going to rehybridize the s in this p orbital piece, right? It's still going to have those 2 p's, those 2, 2 p's, right? You know that already, because a triple bond is what? Three bonds, right? So one, two of them are made by what kind of orbital? P orbital. P orbital, right? So let's fill this stuff up, okay? So how many electrons do we have going in? Four. Four, right? So how are they going to fill? So one, two, and then these ones are going to go up there when those two get filled, or when those two formed, okay? Because the sigma bonds will happen first, okay? So you're going to have a sigma bond with your 1s orbital with your h, and your sp orbital with your n, too. Your n's going to be sp-hybridized, too, okay? So these sigma bonds will happen first, and then these pi bonds will happen next, okay? And then in fact, the hybridization for the nitrogen looks very similar to this. That's a tough question. Yeah.