1. Spin Electronic charge in motion - A current loop behaves as a magnetic dipole and has a magnetic moment. - Note the current direction is opposite to the electron velocity, and also the angular momentum direction is opposite to the magnetic moment Two contributions to the electronic magnetic moment -An orbital magnetic moment due to orbital angular momentum -A spin magnetic moment due to electron spin

2. Electronic Magnetic Moments -Orbital Contribution The orbital motion of an electron around the nucleus may correspond to a current in a loop of wire having no resistance where m=(area of loop) (current) Note that the angular momentum is continuous (not quantized), indicating a classical treatment of the problem

3. Electronic Magnetic Moments -Spin Contribution Spin? - Was postulated in 1925 by Paul Dirac in order to explain certain features of optical spectra of hot gases subjected to a magnetic field(Zeeman effect) and later theoretical confirmation in wave mechanics - The root cause of magnetism and an intrinsic property, together with charge and mass, of subatomic particles of fermions (eg.electrons, protons and neutrons) and bosons (photons, pions) It was found, theoretically and experimentally, that the magnetic moment due to electron spin is equal to,m 0

4. Electronic Magnetic Moments -m vs. p For a given angular momentum, the spin gives twice the magnetic moment of orbit

5. Electronic Magnetic Moments -Total Moments The total magnetic moment per electron is the vector sum of the orbital and spin magnetic moments The term ‘g’ is called the Lande splitting factor — g=2 for spin only components — g=1 for orbital only components

6. Electronic Magnetic Moments -Lande’Equation Orbital is quenching : L=0, J=S  g=2 Spin =0 : S=0, J=L  g=1

7. Schrodinger Equation

8.  m =  hm l m l = l(l+1)

9. Schrodinger Equation

10. Electronic Magnetic Moments -Quantum Mechanical The orbital angular momentum quantum number ( l ) The spin angular momentum quantum number ( l )

11. Hund’s Rule Empirical rules which determine the occupancy of the Available electronics within an atom Used to calculate L, S and J for an unfilled shell 1. Maximum total S=max S z with S z = i m si Obeying the Pauli exclusion principle 2. Maximum total L=maxL z with L z =  i m li Minimizing the Coulomb interaction energy 3. Spin-orbit interaction: L -S  if less than half-filled J= L+S  if more than half-filled

12. Hund’s Rule - Examples Sm 3+ ion having 5 electrons in its 4f shell (n=4, l=3)  S=5/2, L=5, J=L-S=5/2 m l 3 2 1 0 –1 –2 –3 m s occupancy s Fe 2+ ion having 6 electrons in its 3d shell (n=3, l=2)  S=2, L=2, J=L+S=4. Actually, however, S=2, L=0 (quenched) J=S=2 m l 2 1 0 –1 –2 2 1 0 -1 -2 m s occupancy s