The maximum number of orbitals that may be associated with the quantum numbers n = 5 and l =
2 is
So i got 9 for this question, but was marked wrong, and I am not quite sure why? Thanks in advance
I'm not Bob Pursley but will I do.
If you have an s electron, l = 0
If you have a p electron, l - 1
If you have a d electron, l = 2
There are 5 d orbitals.
I suspect you counted the 5d orbitals as well as the 5p(three of those) and the 5s(1 of that) for 6+3|1 = 9.
I've reposted and corrected the three typos.
If you have an s electron, l = 0
If you have a p electron, l = 1
If you have a d electron, l = 2
There are 5 d orbitals.
I suspect you counted the 5d orbitals as well as the 5p(three of those) and the 5s(1 of that) for 5+3+1 = 9.
The maximum number of orbitals that may be associated with the quantum numbers n and l can be calculated using the formula 2l + 1.
For n = 5 and l = 2, plugging these values into the formula:
2l + 1 = (2 * 2) + 1 = 4 + 1 = 5.
Therefore, the maximum number of orbitals for n = 5 and l = 2 is indeed 5. It seems like your answer of 9 may have been incorrect. Double-check your calculations to make sure you didn't make any errors.
To determine the maximum number of orbitals associated with the quantum numbers n = 5 and l = 2, you need to use the following formula:
Maximum number of orbitals = (2l + 1)
In this case, l = 2, so the formula becomes:
Maximum number of orbitals = (2 * 2 + 1) = 5
Therefore, the correct answer should be 5, not 9. It seems there might have been an error in your previous answer or a mistake made during grading.