Question #a7fdc

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Question #a7fdc

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Answer 1 · 2018-02-07T00:59:34

$m_{l} = 0$ $m_l = 0$

Explanation:

Start by writing the electron configuration of a neutral sodium atom.

$Na: 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$ $"Na: " 1s^2 2s^2 2p^6 3s^1$

The last electron in a neutral sodium atom is added to the $3 s$ $3s$ subshell, which, as you know, contains a single orbital, the $3 s$ $3s$ orbital.

Now, the magnetic quantum number, $m_{l}$ $m_l$ , tells you the orientation of the orbital in which an electron is located inside an atom.

In the case of an $s$ $s$ orbital, the magnetic quantum number can only take one value.

$m_{l} = 0$ $m_l = 0$

This is the case because the value of the magnetic quantum number depends on the value of the angular momentum quantum number, $l$ $l$ .

$m_l = {-l, - (l-1), ..., -1, 0, 1, ..., (l-1), l}$

The angular momentum quantum number tells you the shape of the orbital(s), i.e. the energy subshell in which the electron is located.

An $s$ subshell is denoted by

$l = 0$

which implies that the magnetic quantum number can only take one possible value here.

$l = 0 => m_l = 0$

This tells you that an $s$ subshell contains a single orbital, the $s$ orbital.

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Question #a7fdc

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