Well, your collection of quantum number is no "allowed" for a details electron since of the worth you have for #"l"#, the angular inert quantum number.

The values the angular inert quantum number is enabled to take walk from zero come #"n-1"#, #"n"# being the principal quantum number.

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So, in your case, if #"n"# is same to 3, the worths #"l"# should take room 0, 1, and also 2. Because #"l"# is detailed as having the value 3, this puts it external the permitted range.

The value for #m_l# can exist, since #m_l#, the **magnetic quantum number, varieties from #-"l"#, come #"+l"#.

Likewise, #m_s#, the spin quantum number, has an acceptable value, because it deserve to only be #-"1/2"# or #+"1/2"#.

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

Michael
january 18, 2015

There space 4 quantum numbers which describe an electron in an atom.These are:

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

#l# the angular momentum quantum number. This speak you the type of sub - covering or orbit the electron is in. It takes integral values varying from 0, 1, 2, as much as #(n-1)#.

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

#m# is the magnetic quantum number. For directional orbitals such as p and also d it speak you how they room arranged in space. #m# have the right to take integral values of #-l ............. 0.............+l#.

#s# is the spin quantum number. Put merely the electron deserve to be thought about to be spinning top top its axis. For clockwise spin #s#= +1/2. For anticlockwise #s# = -1/2. This is often shown as #uarr# and #darr#.

In your inquiry #n=3#. Let"s usage those rules to view what worths the various other quantum numbers have the right to take:

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

If #l# = 0 #m# = 0. This is one s orbitalIf #l# = 1, #m# = -1, 0, +1. This offers the 3 p orbitals. Therefore #m# = 0 is ok.If #l# = 2 #m# = -2, -1, 0, 1, 2. This gives the five d orbitals.

#s# have the right to be +1/2 or -1/2.

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These room all the permitted values for # n=3#

Note that in one atom, no electron can have all 4 quantum numbers the same. This is exactly how atoms are built up and is well-known as The Pauli exclusion Principle.