CHEM 1A Lecture Notes - Lecture 6: Emission Spectrum, Empirical Formula, Magnetic Quantum Number
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Contains no gaps and all wavelengths in the range are observed absorption spectrum: consists of dark lines on bright background. Observes what wavelengths are missing due to absorption by the sample. Electron move from one lower level to a higher level. Atom absorb energy = emit this energy as light. Light pass through a prism creates emission spectrum. If sample emitting light contains only one atom, known as atomic emission spectrum. Each atom has its own emission spectrum. De broglie"s relation: faster electron moves, smaller the wavelength is. = h / mv = h / p. Empirical formula describing the pattern of the visible wavelengths of the emission spectrum. The uncertainty principle: can never observe simultaneously the interference pattern and determine which slit the electron goes through. Can"t measure both velocity and position at same time. Principle quantum number (n): integer that determines overall size and energy of an orbital.
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