so we can look at another kind of bonding and hybridization so let's look at bh3 we draw the lewis structure for this so this is one of those non octets we know that we should get a 120 degree bond angle based on vesper theory so how does this actually come about we see that we have three electron domains on here so what we're going to do is we're going to take on the boron three electron domains and hybridize them so we're going to take the 2s and 2 the two p's and we're going to hybridize them so that we end up forming degenerate sp2 hybrid orbitals and then we have one orbital left over that is still the 2p that is left over on here so this hybridization creates these three sp orbitals so what we're doing just like last time we are taking the linear combination of the s orbital one of the p orbitals and one of the perpendi the other perpendicular p orbitals and then we end up getting three different lobes that kind of look like this so we end up getting our sp hybridized orbital which is our sp2 hybridized orbital which is 120 degrees so if we look at the valence bond theory picture of this we can actually start off with this sp2 hybrid orbital and then we can take the hydrogens and form our sigma bonds over here and that is how we describe the bonding in something like bh3 we can go from something a little bit more com complex if we look at methane and think about methane or in the water complex what were the water molecule what we're looking at is four domains so that means we want to hybridize four different orbitals on here so we're gonna hybridize all of these so we're gonna hybridize all these and we're gonna form the classic sp3 hybrid orbital and we actually hybridize those we will actually form something that looks like this this is in a tetrahedron type configuration so we can once again have this three-dimensional picture of this orbital and remember our water example up here our water example up here starts off with a sp3 so there's four electron domains there so the oxygen is sp3 hybridized which gives us a base structure with a bond angle of 109.5 so this is your oxygen you have two hydrogens over here so this is 109.5 but remember these electron pairs push these a little bit so this squeezes in a little bit to get our predicted 104 104.5 degrees so we expect it to kind of squish in there just a little bit now we can get even more complicated so we're not just gonna have four things bonded to things sometimes you'll have five different things bonded and this comes up to the concept of expanded octets so if we think about another molecule that has some sort of five electron domains around it we're going to go ahead and hybridize five of them so when we think about this in general chemistry we make sure that we can think about the availability of the 3d electrons in our hybridization so if we have five electron domains what we're going to create now is an sp 3 d hybrid orbital and that's going to look something like this so remember here there are five electron domains and this is our trigonal bipyramid and we can predict the bond is going to look something like this so our sp3d if we have six electron domains we can start to think about this we uh this kind of configuration and that's where we get our octahedral kind of uh electron domain configuration and if we're taking our d's and then our p orbitals and our s we're going to take six of these in there to get an sp3 d2 hybridization which will look something like this