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Chemistry 111

Chemistry 111. Sections 10.1 – 10.4 Chemistry 111. Chapter 10 Topics Electromagnetic (Light) Spectrum Spectroscope Bohr Model Quantum Model (Schr ö dinger) Principle Orbital Shape Exclusion Electron Configuration Noble Gas Cores Periodic Table Trends Valence Electrons.

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Chemistry 111

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  1. Chemistry 111 Sections 10.1 – 10.4 Chemistry 111

  2. Chapter 10 Topics Electromagnetic (Light) Spectrum Spectroscope Bohr Model Quantum Model (Schrödinger) Principle Orbital Shape Exclusion Electron Configuration Noble Gas Cores Periodic Table Trends Valence Electrons What we’ll do: Light & Spectrometer Demonstration Bohr Model Animation Quantum Model – Beginning Computerized Orbitals (breath) Quantum Model Extension Periodic Trends Valence Electrons (ns2np5) Chapter 10

  3. Orange647 nm Green575 nm Violet400 nm Red700 nm Yellow585 nm Blue491 nm Electromagnetic Spectrum (Light) • Visible Light (400 – 700 nm)

  4. Electromagnetic Spectrum (Light)

  5. Spectroscope / Spectrometer

  6. Bohr Model of the Atom • View Animations Online • View UV/Visible Spectrum of: • Hydrogen Lamp • Neon Lamp • Mercury Lamps (overhead lights) • Projector Lamp (Incandescent / W) • Fire works.

  7. Quantum Model • Bohr Model works perfectly for Hydrogen • Doesn’t work well for rest of the periodic table. • Refined with the Schrodinger Equation • Still have Bohr Energy Levels • Add “sublevels” – shape of the orbital • Multiple orbitals per sublevel. • 2 Electrons per orbital

  8. Quantum Model - n • Principle Quantum Number (n) • n can be {1, 2, 3, 4, 5, 6, 7} • Corresponds to the ROWS on the periodic table

  9. Quantum Model - Sublevels • Sublevels = Shape • Show Web Site with shapes. http://www.chem.purdue.edu/gchelp/aos/1s.html • Possible Sublevels: • s, p, d, f • # of possible sublevels is same as value of n: • n = 1: s sublevel only • n = 2: s & p • n = 3: s, p & d • n = 4: s, p, d & f • We never need more than f – there aren’t enough stable elements.

  10. Quantum Model – the One s Orbitals • “s” sublevels are “spherical” (round) • These are the Alkali Metal & Alkaline Earth Metals!

  11. Quantum Model – the Three p Orbitals • “p” orbitals are sketched as pear-shapes (middle). • There is one along each axis – x, y, z for a total of 3. • These are the {Al, C, N, O} families, halogens, noble gases. Left: true shape Middle: sketch Right: All at once.

  12. Quantum Model – the Five d Orbitals • 4 of the “d” are 4-petal flowers. The 5th is weird! These are the transition elements! • These are thetransition metals. B: True Shape C & D: Sketch E: The funny one.

  13. Quantum Model – the Seven f Orbitals These are the Lanthanides & Actinides

  14. Summary

  15. Sublevels & the Periodic Table

  16. Team Exercise • This chapter is mainly qualitative • We will use the team activity to actively review the topics. • Discuss what you don’t fully understand. • Note topics that you want me to go over. • Review your chapter notes. • Update them with good ideas from teammates. • GOAL / ASSIGNMENT: Spend time actively reviewing the material. • Complete your active learning log.

  17. Orbitals / Energy Levels • Bigger orbitals have higher energy, electrons want to fill in the bottom levels first. • Filling Order:1s 1s 2s 2p 2s 2p 3s 3p 3d 3s 3p 3d 4s 4p 4d 4f 4s 4p 4d 4f 5s 5p 5d 5f 5g 5s 5p 5d 5f 5g 6s 6p 6d 6f 6h 6i 6s 6p 6d 6f 6h 6i7s 7p 7d 7f 7h 7i 7j 7s 7p 7d 7f 7h 7i 7j

  18. Electron Configuration • On Chalkboard: • Energy Level Diagrams • Shorthand #1: 1s22s23p6… • Shorthand #2: Noble Gas Core

  19. Periodic Trends – Atomic Radii

  20. Periodic Trends – Ionization Energy

  21. Team Exercise Time • This chapter is mainly qualitative • We will use the team activity to actively review the topics. • Discuss what you don’t fully understand. • Note topics that you want me to go over. • Review your cheatsheets • Update them with good ideas from teammates. • GOAL / ASSIGNMENT: Spend time actively reviewing the material. • Complete your active learning log.

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