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Chem 11 – Class Starter

Chem 11 – Class Starter. Please take out your Periodic Table “cut-ups ” and place them on your table If this makes more sense, why are periodic tables laid out the way they are ? Practicality…. Soon… this “alternative” model of the Periodic Table will become very important to us….

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Chem 11 – Class Starter

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  1. Chem 11 – Class Starter Please take out your Periodic Table “cut-ups” and place them on your table If this makes more sense, why are periodic tables laid out the way they are? Practicality…

  2. Soon… this “alternative” model of the Periodic Table will become very important to us…

  3. Intro to Quantum Mechanics Video

  4. Where were were…? Collect the Quantum Revolution Worksheet from the front of the room In about 8 minutes we will review as a class

  5. Unfortunately… • Bohr’s model on worked for one specific molecule… Hydrogen • So what’s so unique about Hydrogen? One electron system • We can’t have a model that works for only one ATOM!

  6. One more thing… Waves vs. Particles • Is light a wave or a particle? • Is an electron a wave or a particle? BOTH ARE BOTH!?!

  7. Wave-Particle Duality

  8. Finally…. the MODERN MODEL of the atom It took several years, several scientists, and some outside the box thinking to develop the current model of the atom…

  9. Video: NOVA - Quantum Mechanics - Probability Density

  10. Population Density of BC If you had to make a bet (non monetary of course) on finding a specific person, when you have no prior knowledge of where they live, where in BC would you choose?

  11. Bohr Theory The electron is a particle that must be in orbital in the atom. Quantum Theory The electron is like a cloud of negative energy or a wave. Orbitals are areas in 3D space where the electrons most probably are. The energy of the electron is in its vibrational nodes- like notes on a guitar string. Photons are produced when high energy nodes change to lower energy nodes

  12. We now not only have shells… We now have subshells within shells… Oh and by the way… even though they are called shells they are ACTUALLY probability densities

  13. S orbitals • Each orbital holds 2 electrons

  14. P orbitals • There are 3 suborbitals • Each contains 2 electrons • Total electrons = 6

  15. D orbitals • There are 5 suborbitals • Each contains 2 electrons • Total electrons = 10

  16. F orbitals • There are 7 suborbitals • Each contains 2 electrons • Total electrons = 14

  17. Next class we will learn to fill these orbits with electrons..

  18. 7p 6d 5f 7s n = 7 6p 5d 4f 6s n = 6 5p 4d 5s n = 5 4p 3d 4s n = 4 3p 3s Energy levels n = 3 The Electron Energy Levels for a Polyeletronic Atom 2p 2s n = 2 Energy Levels n = 1 1s

  19. Homework: • Hebden: Read p. 151-157 Q’s 26-29 odds

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