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Chemistry

Chemistry . Chapter 11 Modern Atomic Theory. 11.4 The Energy Levels of Hydrogen Different wavelengths of light carry different amounts of energy per photon Red light- less energy Blue light- more energy Draw fig. 11.10, p. 328.

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Chemistry

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  1. Chemistry Chapter 11 Modern Atomic Theory

  2. 11.4 The Energy Levels of Hydrogen Different wavelengths of light carry different amounts of energy per photon Red light- less energy Blue light- more energy Draw fig. 11.10, p. 328. Energy levels are quantized- only certain energy levels are allowed. Why?

  3. 11.5 The Bohr Model of the Atom Niels Bohr- Bohr model of atom (only really works for Hydrogen. Why?) Electrons are not really in circular orbits around the nucleus (even though it is convenient to draw them this way) Draw fig. 11.17, p. 329

  4. 11.6 The Wave-Mechanical Model of the Atom E. Schrodinger & L.V. de Broglie- suggested that light has both wavelike and particle-like characteristics Wave-mechanical model-Electrons can behave with wave properties Orbital- a location for where an electron probably is located. Orbitals can contain 0, 1, or 2 electrons. Heisenberg Uncertainty Principle- one cannot know both the location and the velocity of an electron

  5. (Make sure that you have read all of chapter 11, sections 1-6 before proceeding. Go through the bullets at the beginning of the notes and review all scientists and accomplishments.)

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