Atomic and Solid State Physics 300 WS 300

Atomic and Solid State Physics 3/0/0 WS, 3/0/0 SS http: //www. tufreiberg. de/mk/Dokumente/Atomic_and_Solid_State_Physics/ 1

Literature https: //ebookcentral. proquest. com/lib/freiberg-ebooks/reader. action? doc. ID=5378634 2

Outline (atomic physics) 1. Introduction – Evolution of the atomic physics - Dalton principles - First periodic table 2. First experiments in the atomic physics - Discrete nature of the universe - Atomic models - Problem of the classical physics 3. Quantization of the energy - Atomic spectra - Photo-effect - Frank-Hertz experiment - Bohr’s model of atoms 4. Wave-particle dualism - Photo-effect - Compton effect - Diffraction phenomena - Heisenberg’s uncertainty principle 5. Schrödinger’s equation - Explanation of the meaning - Time-dependent and stationary Schrödinger’s equations - Mathematical properties of a wave function 6. Solution of the Schrödinger equation - For a free electron - For an electron in potential well - For an electron in potential of a harmonic oscillator - For an electron at a potential barrier - For hydrogen atom 7. Atoms in magnetic field - Magnetic moment - Spin of the electron - Spin-orbit coupling 8. Ensembles of particles, distribution functions 3

Evolution of the atomic physics Ø Ø 1808 Dalton: Multiple proportions Ø „The pressure of a gas mixture is equal to the sum of the partial pressures of individual components“ Applicable also for the mass of the compounds, which is a sum of the mass of individual “particles”. Ø The first table of atomic weights Dalton’s principles Ø Ø Ø Chemical elements consist of atoms Atoms of the same element possess the same weight Atoms of different elements possess different weights In compounds, atoms are combined in small integer ratios (1: 1, 1: 2, 2: 3), and similar Atoms cannot be created or destroyed 4

Evolution of the atomic physics Ø 1811 Avogadro Molecular theory of gases Ø „Under the same conditions (pressure, temperature), the same volume of any gas contains the same amount of elementary particles. “ Ideal gas law: Émile Clapeyron in 1834 5

Evolution of the atomic physics Ø 1815 William Prout Atomic mass Ø„The relative mass of every atom is a multiple of the mass of hydrogen. ” Ø 1868 Mendeleev Periodic system of elements 6

The first periodic table 7

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Discoveries in the atomic physics Ø Ø Ø Ø Ø 1869 Hittorf: Cathode rays 1895 W. C. Röntgen: X-rays 1896 Bequerel: Radioactivity 1897 J. J. Thomson: Electron identified 1900 M. Planck: E = h 1903 Rutherford: Atomic nucleus 1905 A. Einstein: E = mc² 1913 N. Bohr: Atomic model 1926 E. Schrödinger: Wave equation 1927 Heisenberg: Uncertainty principle 9

Useful formulas v Newton’s law v Impulse v Kinetic energy v Velocity of light v Einstein’s equation 10

Selected natural constants Avogadro’s constant Boltzmann’s constant Planck’s constant Velocity of light in vacuum Rest mass of electron Rest energy of electron Rest mass of neutron Rest mass of proton Atomic weight unit Elementary charge Vacuum permittivity Vacuum permeability Bohr’s atomic radius Bohr’s magneton NA= 6. 02217(4) 1023 mol-1 k. B = 1. 38062(6) 10 -23 JK-1 h = 6. 62620(5) 10 -34 Js ħ = h/2 p = 1. 0546 10 -34 Js c = 2. 997925(1) 108 ms-1 me = 9. 10956(5) 10 -31 kg mec 2 = 0. 51100 Me. V mn = 1. 67482 10 -27 kg mp = 1. 67261(1) 10 -27 kg m(12 C)/12 = 1. 66055 10 -27 kg e = 1. 602192(7) 10 -19 C e 0 = 8. 8542 10 -12 As. V-1 m-1 m 0 = 1/e 0 c 2 = 1. 2566 10 -6 Vs. A-1 m-1 r 1 = 4 pe 0ħ 2/mee 2 = 0. 529166 10 -10 m m. B = ħe/2 me = 9. 2740 10 -24 JT-1 11