atomic theory

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atomic theory

  1. 1. Atomic Theory<br />By: Katelin Troy<br />
  2. 2. Some History:<br />Henry Baquel<br />Found that Uranium ore emitted rays.<br />
  3. 3. Marie and Pierre Curie<br />Worked with radioactivity and discovered three subatomic particles:<br />~ Alpha ()<br /> ~ Beta ()<br /> ~ Gamma (γ)<br />These explain electrical charges in an atom.<br />
  4. 4. J.J. Thomson<br />~ Studied charges in a Cathode Ray Tube.<br />~ Discovered through his experiment that atoms have negatively charged particles.<br />
  5. 5. Robert Millikan<br />~ Worked with charged oil drops in a chamber.<br />~Discovered the charge and mass of electrons and protons:<br /> Electron<br /> - Charge= -1<br /> - Mass= 9.1094 * 10-28 g<br /> Proton<br /> - Charge = +1<br /> - Mass = 1.6726 * 10^-24g<br />
  6. 6. Earnest Rutherford<br />Worked with gold foil experiment<br /> - Charged particles were aimed at Au atoms.<br />Conclusions:<br /> - An atom has a small positive middle, aka the nucleus.<br /> - Most of the volume of the nucleus is taken up by electrons.<br />
  7. 7. Atomic Structure<br />~ Proton (p+)<br />~ Electron (e-)<br />~ Neutron (n)<br />electron<br />electron<br />electron<br />nucleus<br /> ~protons<br /> ~neutrons<br />
  8. 8. Nucleus:<br />~ p+ and n<br />~ most of atomic mass<br />~ small<br />~ positive charge<br />
  9. 9. Outside Nucleus:<br />~ contains e-<br />~ small light particles<br />~ occupy most of volume<br />~ negative charge<br />
  10. 10. Atoms are neutral<br /> ~ Number of e- = number of p+<br />There are 3 electrons in this atom, how many protons are there?<br />
  11. 11. On the Periodic Table of Elements:<br />Atomic Number<br />Symbol<br />Name<br />Atomic weight<br />1<br />H<br />Hydrogen<br />1.0079<br />
  12. 12. Mass Number<br />~ Not on Periodic Table.<br />~ Number of particles in the nucleus.<br />~ Equal to number of protons and neutrons.<br />
  13. 13. Nuclear Symbols:<br />Mass #<br />A<br />X<br />Atomic #<br />Symbol<br />Z<br />Examples:<br />Na<br />Br<br />22<br />80<br />11<br />35<br />
  14. 14. Isotopes:<br />Atoms of the same element with different mass numbers.<br />Example: Hydrogen Isotopes<br />Hydrogen Deuterium Tritium <br />3<br />H<br />H<br />H<br />1<br />2<br />1<br />1<br />1<br />
  15. 15. The End<br />The End<br />
  16. 16. Works Cited:<br />Moore, John, et al. Chemistry The Molecular Science. Belmont, CA: Brooks/Cole, 2011. Print.<br />
  17. 17. Photos and Diagrams Cited:<br />Slide 2: http://www.flickr.com/photos/52307935@N00/291472553/sizes/l/in/set-72157594358781695/<br />Slide 7, 11, 13:<br />Katelin Troy<br />Slide 15: http://www.flickr.com/photos/d-kav/4428566547/sizes/o/in/photostream/<br />

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