# What are the possible values of ML for each value of L?

**value of l**is 2, the allowed

**values of ml**= -2, -1, 0, 1, 2. Therefore, there are five spatial orbitals which can hold electrons in this subshell.

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Simply so, what are the possible values of L for each value of n?

Because **n**=3, the **possible values of l** = 0, 1, 2, which indicates the shapes of **each** subshell.

- Principal shell with n = 1 has one s subshell (l = 0)
- Principal shell with n = 2 has one s subshell and one p subshell (l = 0, 1)
- Principal shell with n = 3 has one s subshell, one p subshell, and one d subshell (l = 0, 1, 2)

Similarly, what value or values of ML are allowable for an orbital with L 2? Therefore, given **l**=**2** , the possible m**l values** are −**2**,−1,0,1,**2** . This tells us that the d subshell contains five d **orbitals**, each with a different orientation ( dyz , dxy , dxz , dx**2**−y**2** , and dz**2** ).

Considering this, what are the possible values of ML when L 1?

Answer: the **possible values of ml** are -**1**, 0 and +**1** because the range of **values** are from -**l** to +**l**.

How many possible combinations are there for the values of L and ML when n 5?

Answer and Explanation: When **n** = **5 l** can be 0, 1, or 2. These **values** correspond to an s, p, d and f orbitals. The m**l values** range from -3 to +3.