What is the maximum number of orbitals that can be identified with the following quantum numbers? n = 3, l = 1

Question

What is the maximum number of orbitals that can be identified with the following quantum numbers? n = 3, l = 1, m = 0

Accepted Answer

An atomic orbital is uniquely designated by a set of three quantum numbers: the principal quantum number ($n$), the azimuthal quantum number ($l$), and the magnetic quantum number ($m_l$).

1.  **Analyze the given values:**
    *   $n = 3$: Indicates the 3rd principal shell.
    *   $l = 1$: Indicates the 'p' subshell ($3p$).
    *   $m = 0$: Indicates a specific orientation within the 'p' subshell (typically the $p_z$ orbital).

2.  **Conclusion:** This unique combination of three quantum numbers ($3, 1, 0$) corresponds to exactly **one** specific orbital.

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