Chapter 11 Lecture Notes

Wednesday, April 12, 2000

Part I: Review of quanta of light and the two mathematical equations: one which relates wavelength and frequency to the speed of light, and the other that relates the energy of light to its frequency.

Part II: Look at the emission spectrum for hydrogen atoms to see the difference between it and a continuous spectrum.

Part III: Look at the emission spectrum for several other elements and ask several questions about what the nature of the hydrogen atom could be to get the type of emission spectrum we observe.

Part IV: Introduction to the Bohr model of the hydrogen atom, and discuss energy levels, the 'orbiting' electron and how an electron can move from one energy level to another.

Part V: An electron orbiting the nucleus in the Bohr model must absorb a specific amount of energy to 'jump' to a higher energy level. The term energy level is discussed further in this segment.

Part VI: In this segment we watch an electron being excited from one energy level (low) to another energy level (higher). exciting an electron to a higher energy level requires the absorption of a photon of light.

Part VII: Introduction of the quantum number n. The interesting arrangement of the energy levels in the Bohr model of the hydrogen atom is also discussed.

Part VIII: The Bohr model of the atom works great for hydrogen, but not so great for helium. Why? The concept of the electron in terms of a wave is discussed.

Part IX: Introduction of the concept of an orbital. The difference between an electron orbiting the nucleus (Bohr model) and the electron occuping an orbital (Quantum Mechanical model).

Part X: Introduction to the energy level diagram for the Bohr model, and the quantum Mechanical model of the hydrogen atom..

Part XI: Levels, sublevels and orbitals what do these terms mean in our Quantum mechanical model of the hydrogen atom.