Question

Which of the following quantum number combinations is not allowed in an atom?

n = 2, l = 0, m subscript l = 0
n = 3, l = 2, m subscript l = -1
n = 6, l = 5, m subscript l = -4
n = 1, l = 0, m subscript l = 1

Answer 1

The last one my friend. m subscript l is comprised between +l and -l: if l is 0 m can only be 0

Answer 2

In fact the orbital l=0 is the energy sublivel 's', shaped like a sphere, (the level m subcript l indicate the orientation in space, and a sphere "l=0" can only have one orientation in 3d space)

Answer 3

n is the principle quantum number can be any whole integer;

\[M _{L} \] = orientation.

L = shape of your orbital

\[s = \pm \frac{ 1 }{2 }\] this is our spin

Answer 4

our spin can either be up or down, and each orbital the box can hold a maximum of 2 electrons.

if you have

If I remember correctly \[m_{L} = \pm l\] so if you have l = 2 for instance m_{L} can take on any value from positive L to negative L.