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Hybridization of atomic orbitals2/21/2023 We know that a P orbital is shaped like a dumbbell, so we're taking three of these P orbitals here. Those S orbitals here, so one S orbital, and Is shaped like a sphere, so we're taking one of All right, let's thinkĪbout the character, or the shape of this new hybrid orbital. And now we have what we're looking for, because now we haveįour unpaired electrons, so carbon can form fourīonds now, and they're equal in energy, so that's SP three hybridization: We create four new, hybrid orbitals. Orbitals, we call this SP three hybridization, so this is We're doing this using one S orbital and three P This from one S orbital and three P orbitals, Some of the S character, and some of the P character,Īnd you're hybridizing them together into brand new orbitals, and since you're taking Orbital this is no longer going to be a P orbital it's going to be a SP three hybrid orbital,Īnd same with these. Them, so this is no longer going to be an S orbital it's going to be an SP three hybrid And these had oneĮlectron in each of them, but we're gonna hybridize P orbitals, like that, so we have our P orbitals here. Promote the two S orbital," so we're gonna take this S orbital, and we're gonna promote it in energy, and we're going to take these P orbitals andĭemote them in energy, so we're gonna lower those So Linus Pauling said, "Let's do something else here: "Let's go ahead and Those electrons are not of equivalent energy, and Opportunity for carbon to form four bonds, however, Up to the two P orbital, so we're in the excited state now. Show that, so we've moved one of those electrons It up to the P orbital here, so let me go ahead and One of these electrons in the two S, and promote That he said was, you could go ahead and take out The electron configuration here, and so to explain this difference, Linus Pauling came up with Here, and everything's of different energies, and so, what we see from the dot structure and experimentally, doesn't quite match up with This implies that carbon would only form two bonds,īecause I have these unpaired electrons right The valence electrons in the outer shell. Here, that would be these four electrons here, If we look at those four valence electrons on our orbital notation In the two S orbital, and then two P two, and so, I'm assuming you already know yourĮlectron configuration, so it would look something like that. It's one S two, so go aheadĪnd put in two electrons in the one S orbital, two S two, go ahead and put in two electrons We look at the electron configuration for carbon, let's go ahead and do that right now. The table over here, let me go ahead and highlight those four valence electrons, those should be equivalent, and if And so the four valence electrons that carbon brought to Like this, with carbon with its four bonds to hydrogen around it, like that, and in methane,Īll of these bonds are equivalent, in terms of things like bond length and energy. One valence electron, and that gives us the Lewis Dot structure. So we go ahead and draw in our hydrogens with Start with carbon, and its four valence electrons,Īnd then we would put hydrogen around that each hydrogen has one valence electron, Want to draw a dot structure for methane, I would We're going to look at the SP three hybridization present in methane and ethane
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