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Published byRolf O’Neal’ Modified over 9 years ago
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TOIPC: EMISSION SPECTRUM
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Flame Test DEMO
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When Matter is heated it gives off light –Example: fire work, pyrotechnics, flame test –The heat energy absorbed by the metal ions excites the atoms’ electrons –The absorbed energy is eventually released in the form of light
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Another example –Example: light bulb –The electrical energy absorbed by the filament excites the atoms’ electrons –The absorbed energy is eventually released in the form of light
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Why do we see colors? Where do they come from? What are they?
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CONTINUOUS (WHITE LIGHT) SPECTRA When normal white light (such as light from the sun or a light bulb) is passed through a prism (or rain drop), the light separates into a continuous spectrum of colors
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PRISM White light is broken into 7 spectral lights, what are they? ROY G BIV
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Originally Scientists (even Newton) thought that light was made up of particles but this couldn’t’ explain why different color were refracted different NOTICE: Violet bends a lot more than Red
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Light made up of waves
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Basic Wave Vocab
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Transverse vs Longitudinal Waves Transverse Longitudinal
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Wavelength vs. Frequency WAVELENGTH = distance light travels to complete 1 cycle FREQUENCY = number of cycles completed in 1 second
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The colors we see have different wave lengths Red = longer wave length Violet = shorter wave length Which one has the higher frequency?,higher frequency,lower frequency Wavelength and Frequency have an inverse relationship
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You can even calc. the Wave Velocity speed of wave in direction is traveling Velocity = wavelength x frequency Velocity =
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Scientists realized that many light waves couldn’t been seen with the naked Electromagnetic Spectrum
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Higher EnergyLower Energy LINK
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THE MYSTERY OF EMISSION- LINE SPECTRUM Solids, liquids, and dense gases emit light of all wavelengths, without any gaps = Continuous Spectrum
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Thin gases emit light of only a few wavelengths = Emissions or Bright Line Spectrum
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Bright Line Spectrum Atoms cannot emit energy continuously, rather they emit energy in precise quantities How does this work –Electrons absorb energy (they get EXCITED) and “jump” to a higher energy level –After a short time, they “fall” back to lower energy level, giving off a specific amount of energy (a quantum of energy) in the form of a photon (light)
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Scientists of the 19 th century quickly figured out that each element generates its own unique set of wavelengths of emissions and absorptions due to it’s unique electron configuration. Hydrogen:
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Neon line spectra
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