Shell, subshell, and orbital

[904940852]

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?

[Nicole Nikolov 1K]

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.

[Lourick Bustamante 1B]

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.

[Aya Shokair- Dis 2H]

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!!

[804899546]

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?

[Angel R Morales Dis1G]

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.