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4-3 Another Look at the Atom Line Spectra A spectrum that contains only certain colors, or wavelengths, is called a line spectra. All elements emit light when vaporized, or electricity passed through. Atoms absorb energy, then give it off in the form of light. Each element has a unique line spectra. Also referred to as emission spectra Sample Emissions The Bohr Model of Hydrogen Atom Why do elements emit different wavelengths of radiation? Bohr realized that the wavelengths had to do with quantized energy proposed by Planck. Electrons in the atom are quantized Each orbital has different energies. When energy is absorbed electrons jump up in energy levels, when released energy is given off as light Each energy level was labeled by the quantum number , n n =1 was the lowest energy state n= 2 a more excited state…..and so on. Using Planck’s equation E = hv Calculated frequency Matched for Hydrogen only Bohr’s Model His model was only able to accurately predict for Hydrogen with one electron. Matter Waves Planck and Einstein described light as consisting of photons – or quanta of energy. Light travels as a wave Light interacts with matter as a particle Does matter have a duel nature as well? De Broglie referred to this as matter waves Later scientists noticed patterns in electrons that had been reflected from metals after being bombarded. Heisenberg Uncertainty Principle The position and momentum of a moving object can not simultaneously be measured and known exactly. Due to the duel nature of matter and energy Only important with small scale objects For example, This means that we cannot know for sure where an electron is at any given time within an atom. We can only know the probability of finding an electron, not its exact location. Orbital – a 3-dimensional region around the nucleus that indicates the probable location of an electron.