Why there is no 2d and 3f orbitals
Answers
If you are sticking to syllabus then consider the following :-
n - principal quantum number
n takes values from 1 to infinity
n corresponds to shell
q - azimuthal quantum number
q takes values always from 0 to n-1
q correspond to sub-shell
sub-shell were found by ZEEMAN-STARK EFFECTS
I am not going to give details here......
q = 0 s sub-shell
a = 1 p sub-shell
q = 2 d sub-shell
q = 3 f sub-shell
q = 4 g sub-shell
And so on.....
m - magnetic quantum number
m takes values from - q to + q....
m corresponds to orbitals
For example n=2, q=0,1
Now q=1 is p sub-shell
So m=-1, 0,+1
These numbers indicate the degenerate orbital 2px, 2py, 2pz......
Magenetic quantum number is to take with orientation of orbitals in space through which they create magnetic fields
I am not going to give details here....
s - spin quantum number
s takes value - 1/2, +1/2 according to the sense of spinning of electrons on their axis.... Each orbital can accommodate only 2 electrons by Polli's principle.....
So by hunds rule the two electrons in each orbital have opposite spin quantum number....
So not making things complicated 2d orbital means n=2 and q=2
But if n=1,
q =0,1 so q not equal to 2
Hence 2d orbitals are absent.....
Similarly 3f orbitals means n=3 and q=3
But if n=3,
q =0,1,2 so q not equal to 3
Hence 3f orbitals are absent......
For clearing your doubts study through JD LEE INORGANIC CHEMISTRY.......
Sorry for any information which I can't provide here....
Above things are mathematical but in actual it has to take something with energy that 2d and 3f orbitals are absent.....
Again no details as it's out of the syllabus.......
NISHANT ABHANGI
JEE ADVANCED 2019 AIR 6
Answer:
That's great Nishant Bro!!
@Topper boy