# Question #c7b21

##### 1 Answer

Here's what I got.

#### Explanation:

For starters, you know that the *angular momentum quantum number*, **energy subshell** in which an electron is located in an atom, depends on the *principal quantum number*,

#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 **energy subshells**, each described by a value of the angular momentum quantum number.

Now, the *magnetic quantum number*, **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.