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III. Quantum Model of the Atom (p. 98 - 104)

Ch. 4 - Electrons in Atoms. III. Quantum Model of the Atom (p. 98 - 104). A. Electrons as Waves. Louis de Broglie (1924) Applied wave-particle theory to e - e - exhibit wave properties. QUANTIZED WAVELENGTHS. A. Electrons as Waves. QUANTIZED WAVELENGTHS. VISIBLE LIGHT. ELECTRONS.

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III. Quantum Model of the Atom (p. 98 - 104)

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  1. Ch. 4 - Electrons in Atoms III. Quantum Model of the Atom(p. 98 - 104) 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. Quantum Numbers 4. Spin Quantum Number ( ms) • Electron spin  +½ or -½ • An orbital can hold 2 electrons that spin in opposite directions. C. Johannesson

  16. 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 C. Johannesson

  17. Feeling overwhelmed? Read Section 4-2! C. Johannesson

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