Given below are sets of quantum numbers for given orbitals. Name these orbitals.
(a) `n=3, l=1` (b) `n=5, l=2` (c) `n=4, l=1` (d) `n=2, l=0` (e) `n=4, l=2`

Given below are the sets of quantum numbers for given orbitals .Name these orbitals a. n = 2 l = 1 m = -1 b. n = 4 l = 2 m = 0 c. n = 3 l = 1 m = +- 1 d. n = 4 l = 0 m = 0 e. n = 3 l = 2 m = +- 2

.What designations are given to the orbitals having (i) n = 2, l = 1 (ii) n = 2, l = 0 (iii) n = 4, l = 3 (iv) n = 4, l = 2 (v) n = 4, l = 1?

Using the s,p,d,f notations, describe the orbitals with the following quantum numbers, (a) n=1, l=0 (b) n=2, l=1 (c ) n=3, l=0 (d) n=4, l=3 (e ) n=5, l=2

The set of quantum numbers, n = 3, l = 2, m_(l) = 0

The following quantum numbers are possible for how many orbitals (s) n = 3, l = 2, m = + 2 ?

Which of the following sets of quantum numbers are correct? n l m n l m

Using s,p,d notations, describe the orbital with the following quantum numbers. (a) n=1, l=0 (b) n=3, l=1 (c) n=4, l=2 (d) n=4, l=3

The set of quantum numbers, n = 2, l = 2, m_(l) = 0 :

Using s, p and d notations, describe the orbitals with following quantum numbers : (a) n=1, l=0 , (b) n=2, l=0 (c) n=3, l=1 , (d) n=4, l=2

Arrange the electrons represented by the following sets of quantum numbers in decreasing order of energy. (i) n=4, l=0, m_(l)=0, s=+1//2 , (ii) n=3, l=1, m_(l)=1, s=-1//2 (iii) n=3, l=2, m_(l)=0, s=+1//2 , (iv) n=3, l=0, m_(l)=0, s=-1//2