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Quantum Model of the Atom

Electrons in Atoms. Quantum Model of the Atom. 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. A. Electrons as Waves.

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Quantum Model of the Atom

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  1. Electrons in Atoms Quantum Model of the Atom

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

  3. A. Electrons as Waves QUANTIZED WAVELENGTHS

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

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

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

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

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

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

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

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

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

  13. C. Quantum Numbers px py pz

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

  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.

  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

  17. Feeling overwhelmed? Read Section 4-2!

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