all right so we can explain bonding through the combination of our atomic orbitals however if we start to think about something like water and we draw the lewis structure for this and we start to think about this overlap of s orbitals on the hydrogens and maybe it's the p orbitals in the oxygens that are overlapping so if we draw our oxygen we know that we can draw our p orbitals we know from our quantum mechanics that a p orbital is 90 degrees to each other so we can take this overlap and take the hydrogen s orbitals and explain the potential bonding in there but let's think about what this bond this model actually means our model actually means is that the bond angle for the hydrogen oxygen hydrogen bond is 90 degrees and that's just wrong if we actually look at our data if we actually look at our data we know that our bond angle is actually right around 104 degrees so this produce to be a problem for our drawings so when we actually have to think about this we have to create new kinds of orbitals in here so our next chapter is about hybridization and your two learning outcomes from hybridization is to go ahead and explain the concept of atomic orbital hybridization and you're also going to determine the hybrid orbitals associated with different molecular geometries so let's just think about the different ideas inside of hybridization hybridization the first one is that they only exist in covalent molecules so you can forget about ionic compounds we're not going to think about that for this class hybrid orbitals are going to have different shapes than the atomic orbitals so remember your atomic orbitals your s is going to be that dumbbell or the sphere the p orbitals are going to be the dumbbells the d's are kind of the clover leafs but these are going to have new shapes and they actually form from linear combinations these are mathematical combinations of the atomic orbitals another idea is each hybrid orbital is going to have the same shape and the same energy so these are these hybridized orbitals are going to be degenerate and we've already talked about vesper theory that this hybridization matches what we've already learned about vesper theory and anytime we have unhybridized orbitals they are going to able to form pi interactions and all of your hybrid orbitals form sigma interactions so when we're talking about hybrid orbitals they're going to create sigma bonds so let's look at one example of this hybridization so let's look at this molecule that we've drawn on here uh based on vesper theory we know that this is going to be a linear molecule with a 180 degree bond angle so that works out just great for for vesper theory and lewis structures but how can we think about this in terms of hybridization so when we look at the carbon atoms we want to think about what it could actually become so in hybridization what we're going to do for this is we're going to take the 2s and the 2p orbital over here and hey we are going to form a hybrid orbital that hybrid orbital is going to be called an sp and there's going to be two of them and then we're still going to have our two p orbitals that are left over so these are able to form the pi bonds and these over here are able to form the sigma bonds so remember if we looked at our atomic orbitals before we see a triple bond here there should be one sigma bond in here and two pi bonds so remember that these are going to form your pi bonds over here your s and p or your sp orbital hybridized orbitals are going to form the sigma bonds over here so if we actually hybridize this s and p orbital what does this actually look like remember we are going to take linear combinations so we look at our carbon atom we look at the 2s orbital and we're going to put on top of this our p orbital so just remember our p orbital has some sort of positive wave character the other side of the lobe has some sort of negative wave character and then if we just arbitrarily choose this as a positive lobe we can see that we can have d uh constructive interference where we have the same signs over here we have constructive interference so we end up getting a orbital that looks like this and then we actually have two of them so this is one of them the other one is just going to be the other side of that and that other side is that other p orbital and that makes perfect sense for the bonding that is happening in this molecule that we have some sort of lobe that looks like this and our hydrogen s orbital can bond over here and the other hydrogen 1s orbital can bond over here and then our hybrid orbitals match what we're expecting with our vesper theory