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Atomic Theory

Atomic Theory. History of the Discoveries Related to the Atom Mr. Kendall. 450 BC 1800 1897 1901 1910 1911 1913. Main Contributors To Atomic Theory. Planck: Quanta, predictable packets of energy. Millikan: Charge on the electron of -1.

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Atomic Theory

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  1. Atomic Theory History of the Discoveries Related to the Atom Mr. Kendall

  2. 450 BC1800 1897 1901 1910 1911 1913 Main Contributors To Atomic Theory Planck: Quanta, predictable packets of energy Millikan: Charge on the electron of -1 Rutherford: atoms have a nucleus Bohr: Proposed a model of an atom Dalton: Wrote an Atomic Theory with 4 main ideas Thompson negative charge in the atom Democritus: Matter made of tiny things called ATOMS 1924 1926 1926 1932 1962 Chadwick: neutrons Debroglie: Matter has a wave-like nature Heisenberg: E- are waves and particles Gell-Mann: Quarks Schrödinger: E- travel in waves

  3. Timeline of Atomic Theory 450 BC 1800’s _________________________________________________________ Dalton: http://www.iun.edu/~cpanhd/C101webnotes/composition/dalton.html proposed 4 components to an Atomic Theory. Democritus: http://www.fortbend.k12.tx.us/campuses/documents/Teacher/2008/teacher_20081003_1616.doc matter was made of “atoms”

  4. Dalton’s Theory: Foundation of Future Investigations • All matter consists of tiny particles. • Atoms are indestructible and unchangeable (Has been modified with recent discoveries in nuclear chemistry) • Elements are characterized by the mass of their atoms. • When elements react, their atoms combine in simple, whole-number ratios. Their atoms sometimes combine in more than one simple, whole-number ratio. http://web.visionlearning.com/dalton_playhouse/ad_loader.html Click the link at home to explore more about experiments related to Dalton’s theory.

  5. Atomic Theory 1897-1920 ___________________________________ Thomson http://highered.mcgraw-hill.com/sites/0072512644/student_view0/chapter2/animations_center.html negative charge in the atom 1897 Planck http://www.science.uwaterloo.ca/~cchieh/cact/c120/emwave.html Quanta 1901 Millikan http://highered.mcgraw-hill.com/sites/0072512644/student_view0/chapter2/animations_center.html charge on e- 1910 Bohr http://www.wwnorton.com/college/chemistry/gilbert/tutorials/ch3.htm#top http://www.chempractice.com/drills/java_Bohr.php quantum model 1913 Rutherford http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/ruther14.swf nucleus 1911

  6. Contributions to Modern Atomic Theory De Broglie Wave nature of matter 1924 _____________________________________ Gell-Mann Quarks 1962 Heisenberg e- is a wave and a particle 1926 Schrodinger e- orbits as a wave 1926 Chadwick neutron 1932

  7. 3 Basic Parts of the Atom.

  8. Types of Quarks Determine Chargehttp://nobelprize.org/educational_games/physics/matter/1.html Quarks = up (+2/3) and down (-1/3) p+ = 2ups and 1 downn0 = 2 down and 1 up +2 +2-1 = +1 -1-1+2 = 0 3 3 3 3 3 3 Gluon forces between quarks

  9. Electrons travel in waves

  10. Electrons are Particles / Photons • Electrons travel in discreet packets called photons. • To describe these unique packets or quantities of energy the term “quanta” is used. • Every element on the periodic table is made up of atoms with a unique signature of spectral lines • http://phys.educ.ksu.edu/vqm/html/emission.html

  11. Predicting the Location of an Electron in an Atom: • Bohr proposed 4 characteristics to consider to predict the location of an electron. • l = the distance from the nucleus • m = the shape of the orbital in which the e- occupies. (s,p,d,f) • n = axis the orbital occupies. (x, y, z) • s =spin of the e- (+1/2 , -1/2)

  12. Distance from the nucleus: • Levels 1-7: When looking at the periodic table, can be determined by the period number. 1 2 3 4 5 6 7

  13. Shape of the Orbital on the x,y,z Axis • The number of electrons in a particular region determines the shape. s shape 2e- p shape 6e-

  14. Shape of the Orbital on the x,y,z Axis d shape 10e- f shape 14e-

  15. Atom with overlapping orbitals

  16. Spin of the Electron • http://www.colorado.edu/physics/2000/applets/a2.html

  17. Do Electrons behave as a particle or as wave? Definition of Light: • http://chemmovies.unl.edu/ChemAnime/DEFLITD/DEFLITD.html

  18. Einstein vs Bohr Bohr: Predictability Einstein: causality If you know the initial conditions and you know the laws of physics, you can figure out the probability of various outcomes happening, but you can never know which one will definitely occur until after it’s over. If you know all the initial conditions of your system and you know the laws of physics, you can figure out exactly what’s going to happen

  19. Electron behavior as it moves to other energy levels. • This emitted energy is equal to the difference between the high and low energy levels, and may be seen as light. Light emission tutorial http://www2.wwnorton.com/college/chemistry/gilbert/tutorials/ch3.htm

  20. Electrons exhibit particle and wave like behavior“Duality”

  21. Particles of the Atom to date: • Nucleus • Protons = p+ = 3 quarks • Neutrons= n0 = 3 quarks • Electron Cloud • Electrons =e- (particle/wave) Held together by a force called : Gluon

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