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III. Quantum Model of the Atom (p. 129-134)

This text explores the quantum model of the atom, focusing on electrons as waves and the concept of quantized energy levels. It covers topics such as the Heisenberg Uncertainty Principle, Schrödinger's Wave Equation, and the four quantum numbers that specify the "address" of each electron in an atom. The text also discusses the formation of orbitals and the spin quantum number.

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III. Quantum Model of the Atom (p. 129-134)

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  1. III. Quantum Model of the Atom(p. 129-134) Ch. 5 - Electrons in Atoms C. Johannesson

  2. A. Electrons as Waves • Louis de Broglie (1924) • Applied wave-particle theory to e- • e- exhibit wave properties QUANTIZED WAVELENGTHS C. Johannesson

  3. A. Electrons as Waves QUANTIZED WAVELENGTHS C. Johannesson

  4. VISIBLE LIGHT ELECTRONS A. Electrons as Waves EVIDENCE: DIFFRACTION PATTERNS C. Johannesson

  5. B. Quantum Mechanics • Heisenberg Uncertainty Principle • Impossible to know both the velocity and position of an electron at the same time C. Johannesson

  6. B. Quantum Mechanics • SchrödingerWave Equation (1926) • finite # of solutions  quantized energy levels • defines probability of finding an e- C. Johannesson

  7. Radial Distribution Curve Orbital B. Quantum Mechanics • Orbital (“electron cloud”) • Region in space where there is 90% probability of finding an e- C. Johannesson

  8. UPPER LEVEL C. Quantum Numbers • Four Quantum Numbers: • Specify the “address” of each electron in an atom C. Johannesson

  9. C. Quantum Numbers 1. Principal Quantum Number ( n) • Energy level • Size of the orbital • n2 = # of orbitals in the energy level C. Johannesson

  10. s p d f C. Quantum Numbers 2. Angular Momentum Quantum # ( l ) • Energy sublevel • Shape of the orbital C. Johannesson

  11. C. Quantum Numbers • n = # of sublevels per level • n2 = # of orbitals per level • Sublevel sets: 1 s, 3 p, 5 d, 7 f C. Johannesson

  12. C. Quantum Numbers 3. Magnetic Quantum Number ( ml) • Orientation of orbital • Specifies the exact orbitalwithin each sublevel C. Johannesson

  13. C. Quantum Numbers px py pz C. Johannesson

  14. 2s 2px 2py 2pz C. Quantum Numbers • Orbitals combine to form a spherical shape. C. Johannesson

  15. C. Johannesson http://www.chem.tamu.edu/rgroup/hughbanks/courses/673/handouts/4f_orbitals.jpg

  16. C. Quantum Numbers 4. Spin Quantum Number ( ms) • Electron spin  +½ or -½ • Draw them as “up” or “down” • An orbital can hold 2 electrons that spin in opposite directions. C. Johannesson

  17. C. Quantum Numbers • Pauli Exclusion Principle • No two electrons in an atom can have the same 4 quantum numbers. • Each e- has a unique “address”: 1. Principal #  2. Ang. Mom. #  3. Magnetic #  4. Spin #  energy level sublevel (s,p,d,f) orbital Electron (up or down) C. Johannesson

  18. C. Johannesson

  19. Feeling overwhelmed? Read Chapter 5! C. Johannesson

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