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Happy Monday!

Happy Monday!.  Electron Configurations!  Last week of 1 st Quarter Lab Reports due WEDNESDAY!! Chapter 3.3 (Part 2) Test = THURSDAY!. Quantum Number. A number that specifies the properties of electrons Every electron has 4 quantum numbers

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Happy Monday!

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  1. Happy Monday!  Electron Configurations!  • Last week of 1stQuarter • Lab Reports due WEDNESDAY!! • Chapter 3.3 (Part 2) Test = THURSDAY!

  2. Quantum Number • A number that specifies the properties of electrons • Every electron has 4 quantum numbers • Most importantly, it specifies the orbital in which the electron is located

  3. Quantum Numbers

  4. Energy Levels, Sublevels, and Orbitals • Energy Levels (represented by principle quantum number - n) • Higher the n, the farther away from the nucleus (More Energy) • Sublevels (s,p,d,f) • Number of sublevels is related to the energy level • Orbitals • Make up sublevels

  5. There are 4 sublevels (& types of orbitals): s, p, d, f

  6. Sooo…. • Energy levelsare made up of.. • Sublevels which are made up of.. • Orbitals!

  7. Another way to see it:

  8. Another way to see it:

  9. Another way to see it:

  10. Orbitals • Orbital: • Most probable location of electrons (90% chance) • Each orbital can hold a maximum of 2 electrons • Each region corresponds to a specific energy level (n) • Sometimes called electron clouds

  11. Orbitals • Described by both a number and a letter • Number – tells the energy level in which the orbital is located • Letter – tells the shape of the orbital • The higher the energy level, the more different shapes that are possible

  12. s-Orbital

  13. p-Orbitals

  14. d-Orbitals

  15. f-Orbitals

  16. Orbitals

  17. Orbitals • How do these orbitals fit together? • Watch this… • And this…

  18. p.4 in Packet O Fun!

  19. p.4 in Packet O Fun!

  20. p.4 in Packet O Fun!

  21. p.4 in Packet O Fun!

  22. Lets put it all together!

  23. Lets put it all together!

  24. Electron Configurations! • An electron configuration is the arrangement of electrons in an atom

  25. Orbital Labels:(examples) • 1s • 2s • 2p • The number tells us the energy level • 3s • 3p • 3d • The letter tells us the orbital shape!

  26. Happy Tuesday!! • Talk about Conclusions • Electron Configurations Lab Report due tomorrow TYPED Chapter 3.3 (part2) Test = Thursday

  27. Aufbau Principle • Electrons fill the lowest-energy orbital first

  28. The order in which orbitals are filled (Aufbau principle) may be also be displayed as an arrow diagram: 1s 2s 2p 3s3p 3d 4s 4p4d 4f 5s 5p5d 5f 6s 6p6d 6f 7s 7p7d 7f 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f

  29. Pauli Exclusion Principle • Two electrons of opposite spins can occupy the same orbital

  30. Hund’s Rule • The number of unpaired electrons is the maximum possible and these unpaired electrons must have the same spin • (Must fill each orbital with 1 electron–all with the same spin–before doubling up).

  31. Orbital Diagram: Lowest Energy Level

  32. Electron Configuration PracticeH

  33. Electron Configuration PracticeHe

  34. Electron Configuration PracticeLi

  35. Electron Configuration PracticeB

  36. Electron Configuration PracticeBe

  37. Electron Configuration PracticeO 2p 2s 1s

  38. Electron Configuration PracticeNe

  39. Electron Configuration PracticeS

  40. Electron Configuration PracticeCa

  41. Electron Configuration PracticeF

  42. Electron Configuration PracticeFe

  43. Electron Configuration PracticeNa

  44. Electron Configuration PracticeKr

  45. Electron Configuration PracticeAr

  46. Draw a Horizontal Orbital Diagramfor Oxygen: 2p 1s 2s

  47. Draw a Horizontal Orbital Diagramfor Chlorine: • Cl: 1s22s22p63s23p5 2p 1s 2s 3p 3s

  48. Complete bottom of p.11 • Write configurations out based on section above.

  49. Remember the Arrow Diagram: 1s 2s 2p 3s3p 3d 4s 4p4d 4f 5s 5p5d 5f 6s 6p6d 6f 7s 7p7d 7f 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f

  50. Practice using it! • Follow the arrows to write on the electron configurations on the bottom of p.12

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