Okay so what I mean by that is that L is going to range from your positive and the negative L Or the other way around but basically you want to stay within the range of L the negative to the positive. And if it's equal to three we're talking about F Now what is ML ML is the sub orbitals of L. And we're talking about P at L equals two then we're talking about D. So if you have L equals 0 that's as if it's one. Also something that we should know about l is the number corresponds to the shape of the orbital. And then l one thing that we should know is that L What's it n minus one or less basically L cannot equal n. So the higher the number n the further away from the nucleus l is telling us the shape of the orbital which we'll see in the next page I tried to draw out for you. N is telling us what level we're at how far away from the nucleus. So what These orbitals allow us to do is to kind of just have an idea of where the electron is. M equals 0 and MS equals negative 1.5 So why exactly are we trying to figure this out and what is everything mean well according to Heisenberg's uncertainty principle is impossible to determine the exact location and momentum of an electron at a specific point in time single point in time.
Now the question states give the corresponding atomic orbital designations for the electrons with the following quantum numbers.
ATOMIC ORBITALS FREE
So if you have any questions after this feel free to message me or any other chemistry tutor on check will be happy to help. And just know that it's not everything there's a lot to atomic orbitals. There's some background information I'm going to cover before. The topic I'll be covering today is atomic orbitals.
/GettyImages-1182226073-6a7270341f7a4f67bfd9397415ee08ab.jpg "atomic orbitals")
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