5.61 Physical Chemistry 23-Electron Spin page 1 ELECTRON SPIN Experimental evidence for electron spin Compton Scattering (1921): AH Compton suggested that “the electron is probably the ultimate magnetic particle.” SternGerlach Experiment (1922): Passed a beam of silver atoms (4d105s1) through an inhomogeneous magnetic field and observed that they split into two beams of space quantized components. Uhlenbeck and Goudsmit (1925) showed that these were two angular momentum states – the electron has intrinsic angular momentum – "SPIN" angular momentum Pauli Exclusion Principle (1925): no more than 2 electrons per orbital, or, no two electrons with all the same quantum numbers. Additional quantum number, now called ms, was postulated. Postulate 6: All electronic wavefunctions must be antisymmetric under the exchange of any two electrons. Theoretical Justification Dirac (1928) developed relativistic quantum theory & derived electron spin angular momentum Orbital Angular Momentum L = orbital angular momentum L = � l (l + 1 ) l = orbital angular momentum quantum number l ≤ n −1 Lz = m � m = 0, ±1, ±2, …, ±l 5.61 Physical Chemistry page 2 23-Electron Spin Spin Angular Momentum S ≡ spin angular momentum S = � s (s + 1 ) = � 3 2 s = spin angular momentum quantum number s =1 2 Sz = ms � ms = ± 1 2 Define spin angular momentum operators analogous to orbital angular momentum operators L2Yl m (θ , φ ) = l ( l + 1) � 2Yl m (θ , φ ) LzYl m (θ , φ ) = m�Yl m (θ , φ ) Ŝ 2α = s ( s + 1) � 2α mαs = Ŝ zα = ms �α l = 0,1, 2,...n for H atom m = 0, ±1, ±2,... ± n for H atom Ŝ 2 β = s ( s + 1) � 2 β 1 Ŝ z β = ms �β 2 s= 1 2 msβ = − always 1 2 Spin eigenfunctions α and β are not functions of spatial coordinates so the equations are somewhat simpler! α ≡ "spin up" β ≡ "spin down" Spin eigenfunctions are orthonormal: ∫ α α dσ = ∫ β β d σ = 1 ∫ α β dσ = ∫ β α d σ = 0 * * * * σ ≡ spin variable Spin variable has no classical analog. Nevertheless, the angular momentum of the electron spin leads to a magnetic moment, similar to orbital angular momentum. 5.61 Physical Chemistry Electron orbital magnetic moment µL = − page 3 23-Electron Spin e L 2me Electron spin magnetic moment µs = − e gS 2me µL = − e� l ( l + 1) ≡ − β 0 l ( l + 1) 2me µs = − e� g s ( s + 1) = − β 0 g s ( s + 1) 2me µLz = − e e� Lz = − m = − β 0m 2me 2me µSz = − e e� gS z = − gms = − β 0 gms ≈ ± β 0 2me 2me g ≡ "electronic g factor" = 2.002322 Total electronic wavefunction has both SPATIAL and SPIN parts. Each part is normalized so the total wavefunction is normalized Ψ ( r, θ , φ , σ ) = ψ ( r, θ , φ ) α (σ ) ψ ( r, θ , φ ) β (σ ) or e.g. for H atom the ground state total wavefunctions (in atomic units) are 12 Ψ 100 1 2 12 ⎛ Z3 ⎞ = ⎜ ⎟ e − Zrα ⎝π ⎠ Ψ 100− 1 2 ⎛ Z3 ⎞ = ⎜ ⎟ e − Zr β ⎝π ⎠ which are orthogonal and normalized. Note the quantum numbers are now nlmmS