Question #9f419

Jun 20, 2017

Here's what I got.

Explanation:

The magnetic quantum number, ${m}_{l}$, tells you the orientation of an orbital located in a given subshell and on a given energy level.

Simply put, the magnetic quantum number tells you the exact orbital in which an electron is located inside an atom.

The value of the magnetic quantum number depends on the value of the angular momentum quantum number, $l$, which designates the subshell in which the electron is located.

In turn, the magnetic quantum number depends on the value of the principal quantum number, $n$, which designates the energy level on which the electron is located.

Now, an $s$ orbital is located in the $s$ subshell and is designated by

${m}_{l} = 0 \to$ represents an s orbital regardless of energy level

A $p$ orbital is located in the $p$ subshell and is desginated by

${m}_{l} = \left(- 1 , 0 , 1\right\} \to$ represent one of the three p orbitals regardless of energy level, as long as $n > 1$

You can thus say that the $p$ subshell contains three $p$ orbitals

• ${p}_{x} \to {m}_{l} = - 1$
• ${p}_{z} \to {m}_{l} = 0$
• ${p}_{y} \to {m}_{l} = + 1$