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Jeroen van den Brink

Orbital degrees of freedom in strongly correlated transition metal compounds. Part I. Jeroen van den Brink. Cargese 2/8/2011. Outline. PART 1. Orbital degrees of freedom: Introduction. Partially filled electronic shells. Atomic wavefunctions -- orbitals.

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Jeroen van den Brink

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  1. Orbital degrees of freedom in strongly correlated transition metal compounds Part I Jeroen van den Brink Cargese 2/8/2011

  2. Outline PART 1 Orbital degrees of freedom: Introduction Partially filled electronic shells Atomic wavefunctions -- orbitals Electron-electron interactions U and JH Mott-Hubbard and magnetism splitting of eg and t2g manifolds spin vs. orbital degrees of freedom

  3. Outline PART 2 orbital representations orbital-orbital hopping orbitals and superexchange quantum compass models The eg Kugel-Khomskii Hamiltonian Symmetries and Degeneracies Order by disorder

  4. PART 1

  5. INTRODUCTION Partially filled atomic shells

  6. Transion metals 3d 4d 5d 4f 5f R(3d) << R(4s) R(4f) << R(6s) Periodic Table of Elements 1s 2s 2p 3s 3p Sc2+ 3d1 Ti2+ 3d2 V2+ 3d3 Cr2+ 3d4 Mn2+ 3d5 Fe2+ 3d6 Co2+ 3d7 Ni2+ 3d8 Cu2+ 3d9 Zn2+ 3d10 Ti: 3d2 4s2 radius wavefunction Ce: 4f1 5d1 6s2

  7. Atomic & Ionic Radii of Elements

  8. High Tc copper oxides, manganites, iron-, cromium-, nickel-oxides….. a Localized orbitals R >>a R a R >> a conventional metals, semiconductors Ra correlated electron systems Do atomic physics first, include translation symmetry later Small overlap of neighboring atomic wave functions: ‘Electrons spend a long time on one atom and hop around infrequently’

  9. atomic wavefunctions -- orbitals

  10. Hydrogen atom single electron states wikipedia

  11. Hydrogen atom In multi-electron atoms degeneracy of s, p ,d , f states with same n is lifted wikipedia

  12. Zeff 3+ 2+ Li+ H+ 1+ r(1s2) attractive nuclear charge is well-screened (Lithium 3+  ~1+) attractive nuclear charge screened less efficiently Screening of nuclear charge Fill 1s with two electrons next electron into 2s or 2p orbital? we know the answer: lithium 1s22s why? the 1s2 core screens nuclear charge 2p orbital mostly outside 1s2 core 2s: considerable weight inside 1s2 core Aufbau principle: 1s2s 2p 3s 3p 3d 4s For 3d screening is so efficient that in TM atoms 4s already filled while 3d partially empty

  13. Zeff 3+ 2+ Li+ H+ 1+ r(1s2) 4f: (lanthanides) very localized Kondo-lattice models 3d: (row 4 transition metals) 5f: (actinides) between localized and delocalized Mott-Hubbard models 4d & 5d TM’s rather delocalized Mott-Hubbard Contraction of orbitals How can 3d electrons profit from large effective attractive potential close to the nucleus? 3d orbitals contract Can 3s orbitals contract too? No, because radial nodes of 3s are fixed by orthogonality to 1s and 2s 3d can contract because angular wavefunction is orthogonal to filled orbitals 4d & 5d therefore cannot contract much further.... ...but 4f orbitals contract very much (can even be inside the core) strong L•S

  14. These orbitals are NOT the spherical harmonics Ylm 1s 2s 3s 4s 2p 3p 3d 4d 4f

  15. real wavefunctions: spherical coordinates: orbital doublet orbital triplet l=2 d-orbitals

  16. 3d

  17. electron-electron interactions

  18. U JH Coulomb exchange many-electron states electron-electron interactions ^ ^ ^ Full Hamiltonian: H = HKE + H2

  19. Large Atomic Hund’s rule exchange JH Electron Spins Parallel 3d orbitals of e.g. a Mn-ion Large Coulomb interaction U between electrons on the ion • eg orbitals • t2g orbitals

  20. correlation effects -- Mott-Hubbardand magnetism

  21. U = 0 Bands: Metallic behaviour U >> t Mott-Hubbard Insulator Antiferromagnetism AFM state: FM state: E = 0 E = -t2/U Hubbard model Consider array of Hydrogen atoms Hopping amplitude: t Coulomb interaction: U

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