Let's go back down here and let me draw up a dot We now know that both of these carbons in a acetylene are SP hybridized. Let's go back up here to this picture of acetylene. Increase in S character, you're going to get shorter bonds because you have smaller Here has an increased electron density closer to the nucleus, which is one way to think Increased electron density closer to the nucleus for an S orbital than for a P orbital, that means that this lobe On the video on SP3 hybridization, we're talking about 25% S character The video on SP2 hybridization, we talked about 33% S character and then for these hybrid orbitals, we have even more S character, up to 50% and since the electron density for an S orbital is That means it's 50% S character and 50% P character and this is more S character than in the previous videos. When we draw our picture, only think about thisīigger frontal lobe here. Let me go ahead and draw inĪn SP hybrid orbital here and once again, we're going ![]() Two orbitals together to give us two new hybrid orbitals. We took one P orbital, which is shaped like a dumbbell and we hybridized these Once again, we know an S orbital shaped like a sphere. Let's get a little bit of room down here. This carbon right here is SP hybridized since it bonded to two atoms and this carbon right here This is SP hybridization because our new hybrid orbitals came from one S orbital and one P orbital like that. This is no longer a P orbital because we're going to hybridize it to form our SP hybrid orbital. We have carbons, four valence electrons but this is no longer an S orbital because we're going to hybridized it with a P orbital to makeĪn SP hybrid orbital. That's gonna leave behind two P orbitals. We're going to demote a P orbital, only one P orbital this time. We're gonna promote an S orbital in terms of energy and One, two, three and four and we're looking for two hybrid orbitals since carbon is bonded to two atoms. We have carbons, four valence electrons represented here in the excited stage. To find our new type of hybridization, we look at our electronic configuration already in the excited stage. We have a different geometry, a different bond angleĪnd a different number of atoms that this carbon is bonded to. These bond angles are 180 degrees and so we must have aĭifferent hybridization for this carbon. We have carbon bonded to only two atoms and the shape of the acetylene molecule has been determined to be linear. ![]() This carbon is bonded to a hydrogen and it's also bonded to another carbon. If I look at this carbon right here and the ethyne or the acetylene molecule. ![]() Type of hybridization that's present when carbon Is bonded to three atoms and in this video, we're gonna look at the Voiceover: The video on SP3 hybridization, we saw a carbon is bonded to four atoms and in the video in SP2 hybridization, we saw that carbon
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