![]() And then you have the bonding which is a lower energy one and the antibonding which is the higher energy you want. And then you have some key points here, so the number of molecular orbitals is going to be equal to the number of atomic orbitals so if you have all together six atomic orbitals you're gonna get six molecular orbitals. Okay, so here I've just summarized it for you, again for your notes, what I've been talking about, so you get close enough, you get the atomic orbitals, they reshape the molecular orbitals. And each orbital can only accommodate two electrons. You'd fill up at each atomic orbital, you put two electrons in, and the two electrons have to be of opposite spin. And then if you want to say this is a hydrogen, you'd have one electron on each of the hydrogens, and then you'd fill them up just like you learned in school. The way you usually write this is you have an energy level diagram, here you have you two atomic orbitals on each side, and then you have a lower energy bonding molecular orbital and you have a higher energy antibonding molecule. So then, this is just an energy level diagram. You have an antibonding combination, and here I just elaborate on this for your For your notes. So that's the basic principles of Molecular Orbital Theory. So that's an unstable a situation, two positive charges and none of the electrons then shield them from each other, and also there is a much more confined space to like for the electron density. You have no electron density in the middle between the two nuclei. And that electron density can spread out. And here you've got electron density here. Because it's got an electron behavior the two nuclei they're positive charged. So they cancel out and you get an empty one in combination. #Classify these atomic orbitals plusYou have the plus and the negative parts together. As the two waves destructively interfere here in the middle. So you put a minus one here, and then you get this antibonding. So right here you're adding plus plus, but you can also say plus minus. And when they come together for the sigma, for the one S, we call that a sigma. So that's what's called a bonding molecular order. And we know that if you get constructive interference you'll get increased amplitude for the wave and therefore in these two one has orbitals come together. So what they can do then, ways they can combine together. That's why we put a plus or minus on these orbitals sometimes. So like any wave, if you have a sine, a typical wave that you're familiar with, you have positive and negative parts and the same thing for these. Function that comes after the shown equation. So this is three dimensional, this is spherical shaped for an s orbital, is a three dimensional representation of the wave. And these come from the solution of the equation for the hydrogen atom. And they're waves, that's why I put this plus sign here. These are just mathematical descriptions. Sometimes, student, in school especially, have this idea that orbitals are little boxes and electron are little contacts that reside in them. And the idea behind all of these is that they, I hope you now realize that electrons don't reside in boxes. And they combine to give you, you kinda push them together if you like, to give you two molecular orbits. So here the simplest case is hydrogen, so you have the 1s orbitals. But just a recap, you have the idea of a molecular orbital is that you have two atomic orbitals. ![]()
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