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The set of quantum numbers, n = 2, l = 2, m_(l) = 0 :
What is the maximum number of orbitals that can be identified with the following quantum numbers ? n = 3, l = 1, m_l = 0 .
An electron in an atom can be completely designated with the help of four quantum numbers. Out of these, the first three i.e., principal (n), azimuthal (l) and magnetic (m) quantum number are obtained from the solution of Shrodinger wave equation while the spin(s) quantum number arises from the spin of the electron around its axis clockwise or anticlockwise. Of these principal quantum number tells about the size, azimuthal quantum number about the shape and magnetic quantum signifies the orientation of the electron orbital. How many electrons in a given atom have the following set of quantum numbers? n = 3, l =2, m = +2, s = -1//2
Electrons will first enter into which set of quantum numbers-n = 5, l = 0 or n = 3, l = 2
What is the maximum number of electrons that can be associated with a following set of quantum numbers ? (n = 3, l = 1 and m = -1) .
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
In how many elements the last electron will have the following set of quantum numbers, n = 3 and l = 1?
What is the maximum number of orbitals that can be identified with the following quantum numbers? n =3, l= 1, m =0
For how many orbitals are the quantum numbers n = 3, l = 2, m = +2 possible?
Using s,p, d, f notations describe the orbitals with the following quantum numbers: n=3, l= 0, m= 0
