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Electron Configuration & Orbitals

Quantum Model of the Atom. Electron Configuration & Orbitals. Ch. 4 - Electrons in Atoms. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 …. Quantum Model of the Atom. Ch. 4 - Electrons in Atoms.

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Electron Configuration & Orbitals

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  1. Quantum Model of the Atom Electron Configuration & Orbitals Ch. 4 - Electrons in Atoms 1s22s22p63s23p64s23d104p65s24d104p65s24d105p66s24f145d106p6…

  2. Quantum Model of the Atom Ch. 4 - Electrons in Atoms Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  3. Electrons as Waves • Louis de Broglie (1924) • Applied wave-particle theory to electrons • electrons exhibit wave properties Louis de Broglie ~1924 QUANTIZED WAVELENGTHS Standing Wave Fundamental mode Second Harmonic or First Overtone 200 150 100 50 0 - 50 -100 -150 -200 200 150 100 50 0 - 50 -100 -150 -200 200 150 100 50 0 - 50 -100 -150 -200 0 50 100 150 200 0 50 100 150 200 0 50 100 150 200 Adapted from work by Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  4. Electrons as Waves QUANTIZED WAVELENGTHS Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  5. VISIBLE LIGHT ELECTRONS Electrons as Waves Evidence: DIFFRACTION PATTERNS Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem Davis, Frey, Sarquis, Sarquis, Modern Chemistry2006, page 105

  6. Quantum Mechanics • Heisenberg Uncertainty Principle • Impossible to know both the velocity and position of an electron at the same time Werner Heisenberg ~1926 g Microscope Electron

  7. Quantum Mechanics • SchrödingerWave Equation(1926) • finite # of solutions quantized energy levels • defines probability of finding an electron Erwin Schrodinger ~1926 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  8. Orbital Quantum Mechanics • Orbital (“electron cloud”) • Region in space where there is 90% probability of finding an electron 90% probability of finding the electron Electron Probability vs. Distance 40 30 20 Electron Probability (%) 10 0 0 50 100 150 200 250 Distance from the Nucleus (pm) Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  9. UPPER LEVEL Quantum Numbers • Four Quantum Numbers: • Specify the “address” of each electron in an atom Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  10. Quantum Numbers Principal Quantum Number( n) Angular Momentum Quantum #( l) Magnetic Quantum Number( ml) Spin Quantum Number( ms)

  11. Relative Sizes 1s and 2s 1s 2s Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 334

  12. Quantum Numbers 1. Principal Quantum Number( n) • Energy level • Size of the orbital • n2 = # of orbitals in the energy level 1s 2s 3s Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  13. Quantum Numbers y y y z z z x x x px pz py

  14. p-Orbitals px pz py Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 335

  15. s p d f Quantum Numbers 2. Angular Momentum Quantum #( l) • Energy sublevel • Shape of the orbital Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  16. 2s 2px 2py 2pz Quantum Numbers • Orbitals combine to form a spherical shape. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  17. Quantum Numbers n = 1 n = 2 n = 3 Principal level s p s s p d Sublevel dx2- y2 px py px py dxz dyz dz2 dxy pz pz Orbital • n = # of sublevels per level • n2 = # of orbitals per level • Sublevel sets: 1 s, 3 p, 5 d, 7 f Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  18. Maximum Capacities of Subshells and Principal Shells n 1 2 3 4 ...n l 0 0 1 0 1 2 0 1 2 3 Subshell designation s s p s p d s p d f Orbitals in subshell 1 1 3 1 3 5 1 3 5 7 Subshell capacity 2 2 6 2 6 10 2 6 10 14 Principal shell capacity 2 8 18 32 ...2n2 Hill, Petrucci, General Chemistry An Integrated Approach1999, page 320

  19. Quantum Numbers 3. Magnetic Quantum Number( ml) • Orientation of orbital • Specifies the exact orbital within each sublevel Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  20. d-orbitals Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 336

  21. Shapes of s, p, and d-Orbitals

  22. Atomic Orbitals

  23. s, p, and d-orbitals B p orbitals: Each of 3 pairs of lobes holds 2 electrons = 6 electrons (outer orbitals of Groups 13 to 18) C d orbitals: Each of 5 sets of lobes holds 2 electrons = 10 electrons (found in elements with atomic no. of 21 and higher) A s orbitals: Hold 2 electrons (outer orbitals of Groups 1 and 2) Kelter, Carr, Scott, , Chemistry: A World of Choices1999, page 82

  24. Principal Energy Levels 1 and 2

  25. Quantum Numbers 4. Spin Quantum Number( ms) • Electron spin  +½ or -½ • An orbital can hold 2 electrons that spin in opposite directions. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  26. Quantum Numbers • Pauli Exclusion Principle • No two electrons in an atom can have the same 4 quantum numbers. • Each electron has a unique “address”: • 1. Principal #  • 2. Ang. Mom. #  • 3. Magnetic #  • 4. Spin #  • energy level • sublevel (s,p,d,f) • orbital • electron Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  27. Feeling overwhelmed? Read Section 4-2! Chemistry "Teacher, may I be excused? My brain is full." Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  28. Electron Orbitals: Electron orbitals Equivalent Electron shells (a) 1s orbital (b) 2s and 2p orbitals c) Neon Ne-10: 1s, 2s and 2p 1999, Addison, Wesley, Longman, Inc.

  29. O O H H O H H O H H O H H C H H O H H O H H H H What sort of covalent bonds are seen here? (b)O2 (a)H2 (c)H2O (d)CH4

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