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### Shell, subshell, and orbital

Posted: Sun Nov 05, 2017 11:00 pm
What are the maximum and minimum allowable numbers for n, l, and ml. How do I determine this? And if l=3 then does that mean ml= -3, -2, -1, 0, 1, 2, 3?

### Re: Shell, subshell, and orbital

Posted: Sun Nov 05, 2017 11:03 pm
The principal quantum number n simply tells us what energy level the electron is found in. The angular momentum number l describes the shape of the orbital and it can range from 0 to n-1. The magnetic quantum number tells us the orientation of the orbital and ranges from -l to l.

### Re: Shell, subshell, and orbital

Posted: Sun Nov 05, 2017 11:05 pm
The minimum numbers for n and l are 0, but the minimum number for ml would depend on the value of l which can range from 0 all the way to infinity, theoretically. But if applying what we know about energy levels, as energy level n gets larger, the electrons in these energy levels become virtually unattached. And yes, if l=3 then it means ml= -3, -2, -1, 0, 1, 2, 3 because the value of ml is the range from -l to +l including 0.

### Re: Shell, subshell, and orbital

Posted: Sun Nov 05, 2017 11:07 pm
n is any number above 1. So it can be 1,2,3,4....
l is [0,..., n-1]
ml is [-l,l]

So, for example, if you had n=6.
possible values for l=0,1,2,3,4,5. If we pick an electron in the 3 orbital
ml=-3,-2,-1,0,1,2,3

Hope that helps!!

### Re: Shell, subshell, and orbital

Posted: Sat Dec 09, 2017 10:00 pm
For a value of l greater than 4, what would the orbital be? Are there orbitals beyond f orbitals that we don't cover in this class, or is it simply that any l that is 5 or above is considered an f orbital?

### Re: Shell, subshell, and orbital

Posted: Sat Dec 09, 2017 10:13 pm
804899546 wrote:For a value of l greater than 4, what would the orbital be? Are there orbitals beyond f orbitals that we don't cover in this class, or is it simply that any l that is 5 or above is considered an f orbital?

After the f orbital, its the g orbital. We rarely use the f orbital, so using the g orbital is much more rare.