Consider the following quantum number sets; determine if they can occur together
ID: 714809 • Letter: C
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
Explanation / Answer
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