Our new hybrid orbital, let's go ahead and get Notice that we left a P orbital untouched. This carbon right here is SP2 hybridized and same with this carbon. This is SP2 hybridization because we're using one S Orbital and two P orbitals to form This is an SP2 hybrid orbital and same with this one,ДЄn SP2 hybrid orbital. Orbitals has one electron and it's like that. We're gonna take one of the P's and then another one of the P's here. We're gonna promote the S orbital up and this time, we only In this case, we only have a carbon bonded to three atoms. Orbitals and combined them to make four SP3 hybrid orbitals.

In the video on SP3 hybridization, we took all four of these We're gonna start with ourД®lectron configurations over here, the excited stage. A hydrogen, a hydrogen and a carbon and so we must need aДifferent hybridization for each of the carbon's presence in the ethylene molecule. Approximately, 120 degree bond angles and this carbon that I've underlined here is bonded to only three atoms. And the bond angles areД¬lose to 120 degrees. You could think aboutДЄll this in a plane here. Actually, this entire molecule is planar. The geometry of theДЄtoms around this carbon happens to be planar. The carbons in ethenes, let's say this carbon right here, we don't see the same geometry.

Is bonded to four atoms, we have an SP3 hybridization with a tetrahedral geometryДЄnd an ideal bonding over 109.5 degrees. Voiceover: In an earlier video, we saw that when carbon

Sp3d hybrid orbitals