Question

Question #c7b21

Answer 1

Here's what I got.

Explanation:

For starters, you know that the angular momentum quantum number, `l`, which gives you the energy subshell in which an electron is located in an atom, depends on the principal quantum number, `n`.

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

In your case, you have

`n = 3`

which implies

`l = {0, 1, 2}`

This tells you that the third energy level contains a total of `3` energy subshells, each described by a value of the angular momentum quantum number.

Now, the magnetic quantum number, `m_l`, which tells you the specific orbital in which an electron is located, depends on the value of the angular momentum quantum number.

`m_l = { -l, -(l-1), ..., -1, 0 ,1, ..., (l-1), l}`

In your case, you have

• `l = 0 implies m_l = 0`

This tells you that `s` subshell, which is denoted by `l = 0`, contains `1` orbital.

• `l = 1 implies {(m_l = -1), (m_l = 0), (m_l = +1) :}`

This tells you that the `p` subshell, which is denoted by `l= 1`, contains `3` orbitals.

• `l = 2 implies {(m_l = -2), (m_l = -1), (m_l = 0), (m_l = +1), (m_l = +2) :}`

This tells you that the `d` subshell, which is denoted by `l = 2`, contains `5` orbitals.