There are 4 quantum numbers which describe an electron in an atom.
These are:
#n# the principal quantum number. This tells you which energy level the electron is in. #n# can take integral values 1, 2, 3, 4, etc
#l# the angular momentum quantum number. This tells you the type of sub - shell or orbital the electron is in. It takes integral values ranging from 0, 1, 2, up to #(n-1)#.
If #l# = 0 you have an s orbital.
#l=1# gives the p orbitals
#l=2# gives the d orbitals
#m# is the magnetic quantum number. For directional orbitals such as p and d it tells you how they are arranged in space. #m# can take integral values of #-l ............. 0.............+l#.
#s# is the spin quantum number. Put simply the electron can be considered to be spinning on its axis. For clockwise spin #s#= +1/2. For anticlockwise #s# = -1/2. This is often shown as #uarr# and #darr#.
In your question #n=3#. Let's use those rules to see what values the other quantum numbers can take:
#l=0, 1 and 2#, but not 3.This gives us s, p and d orbitals.
If #l# = 0 #m# = 0. This is an s orbital
If #l# = 1, #m# = -1, 0, +1. This gives the three p orbitals. So #m# = 0 is ok.
If #l# = 2 #m# = -2, -1, 0, 1, 2. This gives the five d orbitals.
#s# can be +1/2 or -1/2.
These are all the allowed values for # n=3#
Note that in an atom, no electron can have all 4 quantum numbers the same. This is how atoms are built up and is known as The Pauli Exclusion Principle.