Well, your set of quantum numbers is no "allowed" because that a specific electron due to the fact that of the worth you have actually for #"l"#, the angular inert quantum number.

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

You are watching: What values of l are possible for n = 3?

So, in her case, if #"n"# is equal to 3, the values #"l"# need to take room 0, 1, and 2. Due to the fact that #"l"# is provided as having actually the value 3, this put it outside the allowed range.

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

Likewise, #m_s#, the spin quantum number, has an acceptable 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 allowed for a quantum number is #"l"=3#.

Michael
jan 18, 2015

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

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

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

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

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

#s# is the spin quantum number. Put just the electron deserve to be considered to it is in spinning top top its axis. Because that clockwise turn #s#= +1/2. For anticlockwise #s# = -1/2. This is often shown as #uarr# and also #darr#.

In your inquiry #n=3#. Let"s use those rule to check out what values the other quantum numbers can take:

#l=0, 1 and 2#, however not 3.This gives us s, p and 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# have the right to be +1/2 or -1/2.

See more: Which Results From Multiplying The Six Trigonometric Functions?

These room all the allowed values because that # n=3#

Note that in one atom, no electron can have every 4 quantum numbers the same. This is how atoms are accumulated and is recognized as The Pauli exemption Principle.