Question

Question #03b61

Answer 1

Here's why that is the case.

Explanation:

As you know, we can use a total of four quantum numbers, which make up a quantum number set, to describe the location and spin of an electron in an atom.

The notation used for a quantum number set is

`(n, l, m_l, m_s)`

The quantum number set given to you cannot describe an electron in an atom because the value of the angular momentum quantum number, `l`, which gives you the subshell in which the electron resides, is too high.

As you can see, the angular momentum quantum number can take values in the range

`l = {0, 1, 2, ..., n-1}`

where `n`, which is the principal quantum number, tells you the energy level on which the electron resides.

In your case, you have

`(color(red)(n), color(blue)(l), m_l, m_s) = (color(red)(2), color(blue)(2), -1, -1/2)`

Since `color(red)(n=2)`, it follows that `color(blue)(l)` can only take two possible values

`n=2 implies l= {0, 1}`

Since you have `color(blue)(l=2)`, the quantum number set given to you is not possible for an electron in an atom.