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Evolution of Atomic Structure

Evolution of Atomic Structure. Dalton 1805. Billiard Ball Model Composed of indestructible, indivisible atoms Identical for each element but different from other elements. Thompson 1904. Raisin Bun Model Atoms have electrons embedded in a positive material. Rutherford. Nuclear Model

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Evolution of Atomic Structure

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  1. Evolution of Atomic Structure

  2. Dalton 1805 • Billiard Ball Model • Composed of indestructible, indivisible atoms • Identical for each element but different from other elements

  3. Thompson 1904 • Raisin Bun Model • Atoms have electrons embedded in a positive material

  4. Rutherford Nuclear Model • Atom is composed of a tiny nucleus and orbiting electrons • Most of the atom is empty space • Very small electrons occupy most of the space • Nucleus is composed of protons and neutrons Key experiment: Gold Foil Experiment

  5. http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/ruther14.swfhttp://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/ruther14.swf http://micro.magnet.fsu.edu/electromag/java/rutherford/

  6. Quantum Theory Hot Body Spectrum

  7. Continuous Spectra? • Mathematical model’s could not explain the entire distribution of light at the time • Max Planck surmised that the spectra was not continuous but rather had steps

  8. When specific wavelengths of light hit some metals electrons will be displaced The intensity of the light did not effect the current produced The wavelength of light did effect the current Photoelectric Effect

  9. Quantized Model Electrons exist in exact orbits/shells The distance from the nucleus of each orbit is quantized Used Balmer’s line spectra Bohr Model

  10. http://www.upscale.utoronto.ca/PVB/Harrison/BohrModel/Flash/BohrModel.htmlhttp://www.upscale.utoronto.ca/PVB/Harrison/BohrModel/Flash/BohrModel.html

  11. Types of Spectra

  12. Line Spectra

  13. Bohr’s Postulates Bohr’s First Postulate Electrons do not radiate energy as they orbit the nucleus. Each orbit corresponds to a state of constant energy (called a stationary state). Bohr’s Second Postulate Electrons can change their energy only by undergoing a transition from one stationary state to another.

  14. Quantum Numbers

  15. Principal Quantum Number • Main Shell

  16. The secondary quantum number relates primarily to the shape of the electron orbit. The number of values for l equals the volume of the principal quantum number. Secondary Quantum Number

  17. Magnetic Quantum Number • The magnetic quantum number, ml, relates primarily to the direction of the electron orbit. The number of values for mlis the number of independent orientations of orbits that are possible. • Values of ml range from –l to +l

  18. Spin Quantum Number • The spin quantum number, ms, relates to a property of an electron that can best be described as its spin. The spin quantum number can only be 1/2 or1/2 for any electron.

  19. p. 162 – 184 p. 166 # 1-6, 11 p. 173 #1-5 p. 180 # 1-4, 7, 9, 10 p. 184 # 1-6

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