1. Unit 3, Part 2 Quantum Mechanics Chemistry Notes

3. A Typical Wave http://www.pas.rochester.edu/~afrank/A105/LectureV/FG03_003_PCT.gif

7. The Electromagnetic Spectrum http://www.yorku.ca/eye/spectrum.gif

12. Absorption & Emission Spectra http://www.astro.columbia.edu/~archung/labs/fall2001/images/spectrum_line.gif

13. Hydrogen Atom Example Notice the spectral lines in the same positions? These represent specific energy level changes of the electrons in the atom. http://www.solarobserving.com/pics/hydrogen-spectra.jpg Dark Line Bright Line

14. The Bohr Model http://library.thinkquest.org/19662/images/eng/pages/model-bohr-2.jpg Light Energy Released Light Energy Taken In

16. Ground State vs. Excited State http://imagine.gsfc.nasa.gov/docs/teachers/lessons/xray_spectra/images/emit.gif http://content.answers.com/main/content/wp/en/thumb/c/c4/180px-Energylevels.png Ground State = lowest energy level Excited State = a higher energy level Higher energy levels are closer together…

29. Orbital Shapes http://lincoln.pps.k12.or.us/lscheffler/OrbitalShapesOverheads_files/image002.jpg

31. 3d ___ ___ ___ ___ ___ 4s ___ 3p ___ ___ ___ Principle Energy Level (n) Energy Sublevel (l) Orbital (m) holds 2 electrons total

32. Example Orbital Diagrams 1s 1s2s 1s2s2p http://www.uwgb.edu/dutchs/PETROLGY/WhatElmsLookLike.HTM

37. Electron Configuration Guidelines Place one electron in each orbital before pairing! Degenerate Orbitals: All 3 have the same energy and appear at the same level Hund’s Rule

39. Orbital Filling Clues http://pegasus.cc.ucf.edu/~jparadis/chem2045/chapter06.html