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Quantum Mechanics: Electrons as Waves and Orbital Behavior

Delve into the Quantum Model of the Atom, Louis de Broglie's wave-particle theory, and the fascinating realm of Electrons exhibiting wave properties with quantized wavelengths and visible light interaction. Explore Quantum Mechanics principles such as the Heisenberg Uncertainty Principle, Schrödinger Wave Equation, Radial Distribution Curve, Orbital concept, and the significance of Quantum Numbers in defining electron addresses within an atom. Unravel the mysteries of electron spin, orbital shapes, and the Pauli Exclusion Principle to gain clarity on the behavior of electrons in atoms.

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Quantum Mechanics: Electrons as Waves and Orbital Behavior

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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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