1. Review of Atomic and Quantum Theory Pre Einstein…. Light exhibits Wave Characteristics - Electromagnetic Spectrum, Theory of “Ether” Line Emission Spectrum, Photoelectric Effect - Light/Electrons show Particle Characteristics WAVES PARTICLES http://www.hetemeel.com/einsteinform.php

2. Bohr’s Model of the Atom kosmoi.com/Science/ Physics/Quantum/ kosmoi.com/Science/ Physics/Quantum/ library.thinkquest.org Bohr Model of Atom Electrons can only occupy specific “orbits” Explains Line Emission Spectrums & Quantum Levels Electrons show PARTICLE characteristics

3. The Swinging Pendulum… www.blazelabs.com/ f-p- prop.asp DeBroglie - Explained “particle” nature of Line Emissions with mathematical equations for WAVES. http://dbhs.wvusd.k12.ca.us/webdocs/Galler y/Gallery5.html Light/Electrons show WAVE properties Light/Electrons show PARTICLE properties

4. Remember the Interference Patterns of Waves at Station 4? www.sr.bham.ac.uk/ xmm/diffpage1.html This is a photograph of an a beam of electrons passed through a substance. This is a picture of light being “confined” in a telescope. DeBroglie: A “confined wave”, acts similarly to particles. http://dbhs.wvusd.k12.ca.us/webdocs/Gallery/Gall ery15.html

5. So Where Are They? The Heisenberg Uncertainty Principle Electrons are particles that can be described in terms of BOTH waves and PARTICLES. If you know where the electron is, then you can’t determine its speed or direction. OBSERVATION changes the behavior of the electron If you know the electrons speed and direction, you don’t know where the electron is.

6. Schrodinger www.malaspina.org digg.com/general_sciences/ e=mc%C2%B2_explained Schrodinger developed complex mathematical equations using “quantum numbers “ to describe what Bohr observed but his equations described WAVES not particles.

7. boomeria.org/chemlectures/orbitals/or bitals.html Wait a minute… I don’t buy this! “God does not throw dice! http://www.biografiasyvidas.com/monografia/einstein/fotos/ einstein_1947.jpg

8. http://boomeria.org/chemlectures/orbitals/orbitals.html When Schrodinger put his “quantum numbers” in his equations, mathematically he could calculate the energy levels that Bohr explained with his “planetary” model of the atom.

9. Quantum Energy Levels Energy Levels Quantum Number “n” Quantum “shapes” (sublevel) (Quantum Number “l”)

10. Orbitals http://boomeria.org/chemlectures/orbitals/shapeclouds.jpg

11. Electron Orbitals Example http://fig.cox.miami.edu/~cmallery/150/chemistry/c2x11orbitals.jpg

12. D Orbitals http://www4.nau.edu/microanalysis/Microprobe/img/orbital.jpg

13. 1 Dimensional View of Orbitals www.answers.com/ topic/quantum-mechan

14. Actual Electron Cloud Image of the electron cloud around a nickle impurity in a high-temperature superconductor, obtained with a scanning tunneling microscope. The central spot is the nickle atom, surrounded by a cloverleaf pattern whose fourfold symmetry is indicative of the underlying d-wave nature of the high-temperature superconducting state.PHOTO CREDIT: Seamus Davis/UC Berkeley http://www.berkeley.edu/news/media/releases/2001/06/20_physc.html

15. Electron Configurations Definition - The arrangement of the electrons in an atom. unique to each atom tend to assume arrangements that have the lowest possible energy levels “Ground State Configuration” Defenition - Lowest Energy State arrangement http://hi.fi.tripod.com/timeline/images/electron_cloud.jpg

16. Rules for Defining Electon Configurations Aufbau Principle - an electron occupies the lowest-energy orbital Pauli Exclusion Principle - No two electrons in the same atom can have the same set of 4 quantum numbers. Hunds Rule - orbitals of equal energy have one electron before a second electron is added, and spin direction is the same for single electrons in that energy level.

17. How are Electron Configurations Written Energy Level Comes First… Shape Comes Second… Number of Electrons in the shape comes Third as a superscript… Spin is “implied by # of electrons “1”, “2”, etc. “1s”, “2s”, “2p”, etc. “1s 1”, “ 1s 2”, “ 2s 1”, etc. http://www.beyondbooks.com/psc92/images/00080041.jpg

18. Practical Application Start with Hydrogen… Hydrogen has one electron. Lowest Energy Level is “1” Lowest Energy Shape is “spherical” Lowest Energry Level So… electron configuration will be “1s”

19. Practical Application - Helium Helium has 2 electrons Lowest Energy Level is “1” Lowest Energy Shape is “spherical” Two electrons will occupy orbital with different “spins” Lowest Energry Level So… electron configuration will be “1s 2 ”

20. Electron Configuration Handout Write the Electron Configuration for Hydrogen: Helium: 1s 2s 2p 3s 3p 3d 4s 1s 1s 2

21. Practical Application - Lithium Lithium has 3 electrons Lowest Energy Level is “1” Lowest Energy Shape is “spherical” Two electrons will occupy orbital with different “spins” Next lowest Energy State is level “2” The Lowest Energy Shape at level “2” is spherical So… electron configuration will be “1s 2 2s” Lowest Energy State Second Lowest Energy State

22. Noble Gas Nomenclature When you get to a “Noble Gas”, the electrons fill up all the orbitals on that energy level. You can now describe those electrons with the designation of the Noble Gas in “[brackets]” Example…Lithium can be described as 1s 2 2s or [He]2s since it has all the electrons for Helium plus one more.

23. Practical Application - Beryllium Beryllium has 4 electrons… Beryllium fills up all of the orbitals for “Lithium” then… Adds an additional electron to the same spherical shape as the one Lithium used last So… electron configuration will be “1s 2 2s 2 ” Lowest Energy State Second Lowest Energy State

24. Practical Application - Boron Boron has 5 electrons… Boron fills up all of the orbitals for “Beryllium” then… Uses a new shape, but same energy level. The “p” “shape” can hold up to 6 electrons because of the 3 dimensional orientation. Remember, to NEXT put electrons in each 3 dimensional section of the orbital before putting two together. What rule would this relate to? So… electron configuration will be “1s 2 2s 2 2p” Lowest Energy State Second Lowest Energy State Same Energy Level, different shape

25. Electron Configuration Handout 1s 2s 2p 3s 3p 3d 4s

26. Practical Application - Carbon, Nitrogen, Oxygen, Flourine, Neon Carbon has 6 electrons So… electron configuration will be “1s 2 2s 2 2p 2 ” Nitrogen has 7 electrons So… electron configuration will be “1s 2 2s 2 2p 3 ” What are the electron configurations for Oxygen, Flourine and Neon? Lowest Energy State Second Lowest Energy State Same Energy Level, different shape

27. Electron Configuration Handout 1s 2s 2p 3s 3p 3d 4s Now we are at Argon… What next? Notice that the next lowest energy level is not “3d” but “4s”! Sometimes different shapes have different energy levels than are “lower” than the Quantum number level. So the electron configuration added for Potassium starts at “4s”