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(i) An atomic orbital has n = 3. What are the possible values of l and ml?

(ii) List the quantum numbers (ml and l ) of electrons for 3d orbital.
(iii) Which of the following orbitals are possible? 1p, 2s, 2p and 3f

Chemistry - Main Course Book I

Chapter 2. Structure of Atom



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L = Azimuthal quantum number = varies from 0 to n-1.
         so n = 3  =>  l = 0, 1, 2..  => s , p , d orbitals. in the shell M.

n = 3 and  l = 2      for 3d orbital.
ml = varies from  - l  to  +l    ie.,  -2, -1, 0, 1, 2.  There are 5 magnetic quantum numbers.  That is there are 5 dum-bbell shaped orbitals for the 5 pairs of electrons possible in th d orbital..

1p is not possible as  n = 1.  so  l = 0 only.. ie., only 1s orbital.
2s  is possible.
2p is possible.  as  l = 1 for p orbital.
3f  is not possible as  l = 3  for f orbital...  but n = 3 only.. so l < n..

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