Well, your collection of quantum number is not "allowed" because that a particular electron because of the value you have actually for #"l"#, the **angular momentum quantum number**.

The worths the angular momentum quantum number is allowed to take walk from zero to #"n-1"#, #"n"# being the **principal quantum number**.

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So, in her case, if #"n"# is equal to **3**, the worths #"l"# have to take are **0**, **1**, and **2**. Because #"l"# is noted as having the value **3**, this puts it external the allowed range.

The value for #m_l# deserve to exist, because #m_l#, the **magnetic quantum number, arrays from #-"l"#, come #"+l"#.

Likewise, #m_s#, the **spin quantum number**, has actually an agree value, due to the fact that it have the right to only be #-"1/2"# or #+"1/2"#.

Therefore, the only value in your collection that is not permitted for a quantum number is #"l"=3#.

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Michael

january 18, 2015

There space 4 quantum number which define an electron in one atom.These are:

#n# the primary quantum number. This speak you which power level the electron is in. #n# deserve to take integral values 1, 2, 3, 4, etc

#l# the angular inert quantum number. This tells you the type of below - shell or orbit the electron is in. The takes integral values varying from 0, 1, 2, approximately #(n-1)#.

If #l# = 0 you have an s orbital.#l=1# provides the ns orbitals#l=2# provides the d orbitals

#m# is the magnetic quantum number. Because that directional orbitals such as p and also d it tells you exactly how they space arranged in space. #m# can take integral worths of #-l ............. 0.............+l#.

#s# is the rotate quantum number. Put simply the electron deserve to be thought about to it is in spinning top top its axis. Because that clockwise rotate #s#= +1/2. For anticlockwise #s# = -1/2. This is often presented as #uarr# and also #darr#.

In your question #n=3#. Let"s use those rules to see what worths the various other quantum numbers deserve to take:

#l=0, 1 and also 2#, however not 3.This provides us s, p and also d orbitals.

If #l# = 0 #m# = 0. This is one s orbitalIf #l# = 1, #m# = -1, 0, +1. This provides the three p orbitals. Therefore #m# = 0 is ok.If #l# = 2 #m# = -2, -1, 0, 1, 2. This provides the five d orbitals.

#s# deserve to be +1/2 or -1/2.

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These space all the allowed values for # n=3#

Note that in one atom, no electron can have all 4 quantum number the same. This is just how atoms are collected and is known as The Pauli exclusion Principle.