Question #1b269

1 Answer
Sep 15, 2017

Answer:

Here's why that is the case.

Explanation:

Your quantum number set cannot describe an electron in an atom because the value of the magnetic quantum number, #m_l#, is not permitted given the value of the angular momentum quantum number, #l#.

https://courses.lumenlearning.com/boundless-chemistry/chapter/quantum-mechanical-description-of-the-atomic-orbital/

In your case, you have

#(color(red)(3), color(blue)(2), color(purple)(3), -1/2)#

The electron is said to be located on the third energy level, which has #n=color(red)(3)#, in the #d# subshell, which is denoted by

#l = color(blue)(2)#

For the #d# subshell, the magnetic quantum number is restricted to a total of #5# values

#m_l = {-2, -1, 0, 1, 2}#

As you can see, #m_l = color(purple)(3)# is not possible for an electron located in the #d# subshell #-># this quantum nubmer set cannot describe an electron in an atom.