Question

Consider the following quantum number sets; determine if they can occur together to specify an orbital. If not, indicate which rule has been violated

(a) n=2, l=-1, ml = -1

(b) n=3, l=1, ml=0

(c) n=3, l=3, ml=-3

2: (a) Find all possible subshells in n=4 shell and label these subshells.

2(b): How many total orbitals in shell n=4? what is the relationship between the total number of shell and the quantum number n for that shell?

Please include step-by-step and explanations if possible. I am having a hard time grasping this conce

Answer 1

1)

(a) n = 2, l = -1,    ml = -1

this does not occur. because ' l ' value should not be negative. its always positive or zero.

l = n -1

(b) n=3, l=1, ml=0

this indicates 3p orbital.

(c) n=3, l = 3, ml=-3

this does not occur . because n value and l value should not be equal.

2)

a) n = 4

there are 4 subshells

the corresponding subshells are 4f , 4d , 4p , 4s

b)

if n = 4

number of orbitals = 16

the relation between total number of orbitals = n²