An orbital made of four lobes can have the following quantum numbers
n=2,l = 2, m=0;
n=3,l = 1. m = -2;
n=3,l = 2,m=-1;
n=3,l = 3,m =-3;

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

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

How many electrons in a given atom can have the following quantum numbers ? (a) n = 3, l = 1 (b) n = 3, l = 2, m_l = 0 (c ) n = 3, l = 2, m_l = +2, m_s = + 1/2 (d) n = 3 .

Which orbital represents the following set of quantum numbers n =3, l=0, m =0 s = + 1//2

Describe the orbital with following quantum numbers: (i) n=3, l=2 (ii) n=4, l=3

How many electron in an atom may have the following quantum number ? A n = 4, m_(s) = -(1)/(2) b n = 3,l = 0

The decrerasing order of energy for the electrons represented by the following sets of quantum number is : 1. n = 4,l = 0,m = 0,s = +- 1//2 2. n = 3,l = 1,m = 1,s = - 1//2 3. n = 3,l = 2,m = 0,s = + 1//2 4. n = 3,l = 0,m = 0,s = - 1//2

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

Describe the orbital with the following quantum numbers : (i) n = 1, l = 0 " " (ii) n = 2, l = 1, m = 0 (iii) n = 3, l = 2 " " (iv) n = 4, l = 1 (v) n = 3, l = 0, m = 0 " " (vi) n = 3, l = 1 .