Question

Allowed values for the quantum numbers of electrons are as follows:

n = 1, 2, 3, . . .
l = 0, 1, 2, 3, . . . , n

Answer 1

The quantum no. for all L shell electrons are given below.

For L shell, n=2, Thus for n=2, l = 0,1,

l = 0 corresponds to s subshell. (for l = 0, m = 0)

l = 1 corresponds to p subshell (for l = 1, m = -1, 0, 1)

So the Quantum no. for all s electrons are (in order of n,l,m,s) -

2, 0, 0 (1/2)
2, 0, 0 (-1/2)

The quantum no. for p electrons are ( in order of n,l,m,s) -

2, 1, -1, (1/2)
2, 1, -1, (-1/2)
2, 1, 0, (1/2)
2, 1, 0, (-1/2)
2, 1, 1, (1/2)
2, 1, 1, (-1/2)

d subshell does not exist for L shell.

The quantum no. for M shell electrons-

For M shell n = 3,

l = 0,1,2

for l = 0 , m = 0

for l = 1 , m = -1, 0 1

for l = 2 , m = -2, -1, 0, 1, 2

for l = 0 (s subshell) quantum no. of electrons are -
3, 0, 0, (1/2)
3, 0, 0, (-1/2)

For l = 1 (p subshell)

3, 1, -1, (1/2)
3, 1, -1, (-1/2)
3, 1, 0, (1/2)
3, 1, 0, (-1/2)
3, 1, 1, (1/2)
3, 1, 1, (-1/2)

For l = 2, (d subshell)

3, 2, -2, (1/2)
3, 2, -2, (-1/2)
3, 2, -1, (1/2)
3, 2, -1, (-1/2)
3, 2, 0, (1/2)
3, 2, 0, (-1/2)
3, 2, 1, (1/2)
3, 2, 1, (-1/2)
3, 2, 2, (1/2)
3, 2, 2, (-1/2)