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EMISSION SPECTRUM

EMISSION SPECTRUM

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EMISSION SPECTRUM

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  1. EMISSION SPECTRUM

  2. When Matter is heated it gives off light • 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

  3. CONTINUOUS (WHITE LIGHT) SPECTRA When normal white light (such as light from the sun or a light bulb) is passed through a prism, the light separates into a continuous spectrum of colors

  4. PRISM • White light is broken into 7 spectral lights, what are they? ROY G BIV

  5. Originally Scientists (even Newton) thought that light was made up of particles but this couldn’t’ explain why different color were refracted differentNOTICE: Voliet bends a lot more than Red

  6. Light made up of waves

  7. Basic Wave Vocab

  8. Transverse vs Longitudinal Waves Transverse Longitudinal

  9. Wavelength vs. Frequency • WAVELENGTH = distance light travels to complete 1 cycle • FREQUENCY = number of cycles completed in 1 second

  10. The colors we see have different wave lengths • Red = longer wave length • Violet = shorter wave length ,lower frequency ,higher frequency Which one has the higher frequency? Wavelength and Frequency have an inverse relationship

  11. You can even calc. the Wave Velocity • speed of wave in direction is traveling • Velocity = wavelength x frequency Velocity = 

  12. Scientists realized that many light waves couldn’t been seen with the naked Electromagnetic Spectrum

  13. Lower Energy Higher Energy LINK

  14. THE MYSTERY OF EMISSION- LINE SPECTRUM Solids, liquids, and dense gases emit light of all wavelengths, without any gaps = Continuous Spectrum

  15. Thin gases emit light of only a few wavelengths = Emissions or Bright Line Spectrum

  16. Bright Line Spectrum • Atoms cannot emit energy continuously, rather they emit energy in precise quantities • How does this work • Electrons absorb energy (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)

  17. Scientists of the 19th century quickly figured out that each element generates its own unique set of wavelengths of emissions and absorptions. Hydrogen:

  18. Neon line spectra

  19. Hydrogen jumps!