Question #079e3

1 Answer
Stefan V.
Aug 13, 2016

#m_l = 0#

Explanation:

As you know, a total of four quantum numbers can be used to describe the location and spin of an electron inside an atom.

![figures.boundless.com](useruploads.socratic.org)

The problem wants you to find the value of the magnetic quantum number, #m_l#, associated with an electron located in the #2s^1# orbital.

Now, the magnetic quantum number tells you the exact orbital in which the electron is located. As you can see, the magnetic quantum number depends on the angular momentum quantum number, #l#< which tells you the subshell in which the electron is located.

Simply put, every subshell will have a different number of orbitals as given be

#m_l = -l, ..., -1, 0, 1, ..., l#

A #2s# orbital is located in the s-subshell, which is given by

#l =0 -># the s-subshell

As you can see, the magnetic quantum number can only take one possible value for #l=0#, and that is

#m_l = 0 -># the s-orbital

This tells you that the s-subshell contains a single orbital, the s-oribtal. In this particular case, the #2s# subshell will contain one orbital, the #2s# orbital.

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