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Entry Task: October 16 th -17 th Block 1

Entry Task: October 16 th -17 th Block 1. Question: What is the shape of the p orbitals? How many electrons can a filled p orbital fill? You have 5 minutes!. Agenda. Sign off and discuss section 5-2 Notes on Electron configuration H.W. Section 5-3 ws. Break out periodic Table!!.

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Entry Task: October 16 th -17 th Block 1

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  1. Entry Task: October 16th -17th Block 1 • Question: What is the shape of the p orbitals? How many electrons can a filled p orbital fill? • You have 5 minutes!

  2. Agenda Sign off and discuss section 5-2 Notes on Electron configuration H.W. Section 5-3 ws

  3. Break out periodic Table!!

  4. s= 2 electrons 1s 1s p= 6 electrons 2p 2s 3p 3s d= 10 electrons 4s 4p 3d 4d 5p 5s 6s 6p 5d 7s 6d f= 14 electrons 4f 5f

  5. I can… • Apply the rules to fill in an electron diagram • Write electron configuration for a given element.

  6. Electron Configuration

  7. How do electrons fill the atomic orbitals? There are rules when filling the atoms orbits with electrons.

  8. #1 Aufbau Principle: each electron occupies the lowest energy orbital available. You fill in order of increasing energy. s  p d f Different sublevels have different energy levels. All orbitals in a sublevel have equal energy p > s 2px = 2py = 2pz

  9. #2 Pauli Exclusion Principle • A maximum of 2 electrons are allowed in a single atomic orbital, but only if they have opposite spins!

  10. #3 Hund’s Rule • Fill each sublevel (i.e. all p-orbitals) with single electrons with parallel spins first. Then come back to put 2nd electrons in. First: 2p Think of it as the school bus rule. Fill up the seats singly first then double.

  11. Orbital Shapes

  12. Aufbau Diagram s= 2 electrons p= 6 electrons d= 10 electrons f= 14 electrons

  13. Order of filling electrons

  14. Aufbau Diagram Hydrogen

  15. Aufbau Diagram What rule applies here? Pauli Exclusion- 2 different spins Helium

  16. Aufbau Diagram Lithium

  17. Aufbau Diagram What rule applies here? Aufbau Principle- Fill lower energy levels first Beryllium

  18. Aufbau Diagram Boron

  19. Aufbau Diagram What rule applies here? Hund’s Rule Fill the sublevel first Carbon

  20. Aufbau Diagram Nitrogen

  21. Notations of Electron Configurations • Standard • Shorthand

  22. Aufbau Diagram Fluorine 2p5 2s2 1s22s22p5 1s2

  23. Standard Notation of Fluorine Number of electrons in the sub level 2,2,5 1s22s22p5 Main Energy Level Numbers 1, 2, 2 Sublevels

  24. Shorthand Notation • Use the last noble gas that is located in the periodic table right before the element. • Write the symbol of the noble gas in brackets. • Write the remaining configuration after the brackets. • Ex: Fluorine: [He] 2s2 2p5

  25. START with Hydrogen= put its Electron configuration in its square H 1s1

  26. Helium= put its Electron configuration in its square He 1s2

  27. Lithium= put its Electron configuration in its square Li 1s22s1

  28. Keep Going- until you reach Neon

  29. Neon= put its Electron configuration in its square Ne 1s22s22p6

  30. Orbital occupancy for the first 10 elements, H through Ne.

  31. Sodium= put its Electron configuration in its square- Noticed I put it into shorthand Na [Ne]3s1

  32. Order of filling electrons

  33. The relation between orbital filling and the periodic table

  34. What’s wrong with this configuration? 1s22s22p63p63s2 Correct: 1s22s22p63s23p6 s orbitals are lower energy than p orbitals.

  35. Aufbau Diagram 20 electron Chromium 24 Cr [Ar]4s13d5

  36. Aufbau Diagram 20 electron Copper 29 Cu [Ar]4s13d10

  37. Exceptions to the rules! Cr [Ar]4s13d5 Cu [Ar]4s13d10 WHY?These electron configurations are more stable for the elements!

  38. http://www.chempractice.com/drills/java_AO.php Aufbau Diagram http://www.lon-capa.org/~mmp/period/electron.htm

  39. Blocks in the Periodic Table

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