Sigma and Pi Bonds: Hybridization Explained!

Hey guys, I had a small request for a discussion on the

sigma

and pi

bonds

, almost certainly what they are with respect to carbon. So here's what I need you to know: Sigma

bonds

Between a carbon and anything else is the first bond that carbon forms with any other atom. The first one is always

sigma

, always if carbon forms multiple bonds with an atom, like a carbon-carbon double bond or a carbon-carbon triple bond or something like a carbon-nitrogen triple. I don't care what the second or third link is. It is formed with an atom. Those will be pi links.

Look at this. Here is a picture of a compound I just invented. I even know its name, but The deal is that every first bond is a sigma bond, so here's a bond between carbon and hydrogen. The first is a sigma bond. This is the first one. It's a sigma bond. That one over there, the first one, is a sigma bond, and that is a sigma bond. That is a Sigma Bond. That's the first one. That's the first one That's the first one of these is a sigma bond because one of them is the first bond and that's a sigma bond Every bond that carbon makes with something else is going to be a sigma bond but every second or third bond is a pi link Look, there's a link there One of those links is a pi link, the first sigma the second is Pi Here are two additional links.

There is a second and a third link. One of them is a pi bond and the other is a pi bond. Every first is sigma and every second or third is Pi, so it's easy to tell if it's a sigma or pi bond, but what? Does that even mean it's the real question? Well, here's the deal when it comes to electronic configurations. Sigma bonds are always made of hybridized orbitals, while Pi bonds are made of leftover P orbitals and We decide what the

hybridization

of carbon is based on. How many multiple links does it form? Check it out.

Let's do the three examples. What we're going to do is a carbon that has only single bonds, a carbon that has a double bond, and a carbon that has a triple bond. Let's do all three. Here are carbon atoms with only single bonds, so sigma sigma sigma sigma. These are all sigma links. They are made of hybridized orbitals, so when we hybridize the normal carbon atom we need to have four openings for hybridized orbitals. When this carbon, a carbon that only has single bonds, hybridizes, the 1's are left alone. But the 2, and the peas have to be combined, in fact we need one two three four sigma bonds one two three four which requires one s the 2 and three P So we end up with four Sp.

Three? Hybrid orbitals take our electrons and spread them out and boy, isn't it just convenient? Now we have room for bonds to form one, two, three, four. This is the hybridized electronic configuration for a carbon that only has single, one, two, three, four hybridized bonds. orbitals all sigma bonds When a carbon forms a double bond, however, it forms one, two, three sigma bonds and one Pi bond, the Pi bond being the second bond. This is just an example of a molecule. It could be any molecule that has a double bond like this. I showed you before.

One, two, three hybridized orbitals are needed and one p orbital must be left over. Remember our rule. The Pi bonds are left over from the P orbitals. So when this hybridizes, do you end up with a 1s orbital? one, two, three sigma bonds and to hybridize in three equivalent orbitals we need 1 s and 2 P orbitals and we need to leave one of the 2 P orbitals alone, share it with your electrons 1 2 3 I will not continue I have about the principle or the rule of hund or whatever, but the point here is that it can still form four bonds? one, two, three sigma or single bonds and an opening for a double bond to form.

Any carbon that has a single double bond has this electronic configuration for the hybridized carbon. Finally, what happens when a carbon forms a triple bond or actually forms two double bonds? bonds This is the same case where this carbon has a sigma bond there and a sigma bond here But it has two pi bonds because the second and the third are both Cowntess Pi bonds Here you have a sigma and a sigma This second counts as a pI and this second counts as pI, so in both cases there are two pi bonds being formed that you should already know.

That means you have two p orbitals left over your 1s. It never touches like before and that means two single bonds are being created. You need to hybridize the s with one of the peas. One two three four. Electrons can form two single bonds and two double bonds. Look guys. We really kept up with the Pi sigma orbital

hybridization

rules to explain why carbon bonds the way it does. Why does it have the angles it does and why, to be honest? Why can simple links rotate? But double bonds, right? I haven't

explained

the geometry, but trust me on that.

When a carbon only has single bonds, everyone is sick of us, and it takes four Sp Three hybrid orbitals to do it when you have them. a double bond needs three Sp2 hybrid orbitals for the three single bonds and a leftover P orbital for the double bond or Pi bond. Finally for the triple bond it needs two simple Sp, two simple Sp bonds. Hybrid orbitals for the sigma bonds and you need two orbitals P leftovers. For the two pi links, everything is here. Not the best of fiction's luck.