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== == = = = = = = ="I've Seen Fire and I've Seen Rain"=

Well, your job is to research that question!
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What does it mean for an electron to be excited? How does an electron become excited? What happens when an electron becomes "un-excited"?
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At the end of this Unit, the student should be able to:
 * Describe the composition of the atom and the experiments that led to that knowledge.
 * Describe how Rutherford predicted the nucleus.
 * Describe the composition of the atom and the experiments that led to that knowledge.
 * Describe how Rutherford predicted the nucleus.
 * Explain that Niels Bohr produced a model of the hydrogen atom based on experimental observations. This model indicated that:
 * an electron circles the nucleus only in fixed energy ranges called orbits;
 * an electron can neither gain or lose energy inside this orbit, but could move up or down to another orbit;
 * and that the lowest energy orbit is closest to the nucleus.
 * Recognize the historical contribution that this model gave to our modern theory of the structure of the atom; however, also realize the limitations of this model (applicable only to the hydrogen atom).
 * Describe the wave/particle duality of electrons.
 * Describe the electron cloud of the atom in terms of a probability model.
 * Understand the inverse relationship between wavelength and frequency, and the direct relationship between energy and frequency.
 * Analyze diagrams related to the Bohr model of the hydrogen atom in terms of allowed, discrete energy levels in the emission spectrum.
 * Understand that energy exists in discrete units called quanta.
 * Describe the concepts of
 * an atom being “excited” above its ground state by the addition of energy, resulting in the electron(s) moving to a higher energy level.
 * when the atom returns to its ground state, the electron(s) releases that energy gained as electromagnetic radiation (emissions spectrum).
 * Articulate that this electromagnetic radiation is given off as a photon(s). This photon represents the physical difference between ground state and excited state.
 * Use the “Bohr Model for Hydrogen Atom” and “Electromagnetic Spectrum” diagrams from the Reference Tables to relate color, frequency, and wavelength of the light emitted to the energy of the photon.