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Electromagnetic Spectrum

Electromagnetic Spectrum. The emission of light is fundamentally related to the behavior of electrons. Properties of Light. Visible light is a kind of electromagnetic radiation A form of energy that exhibits wavelike behavior

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Electromagnetic Spectrum

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  1. Electromagnetic Spectrum The emission of light is fundamentally related to the behavior of electrons.

  2. Properties of Light • Visible light is a kind of electromagnetic radiation • A form of energy that exhibits wavelike behavior • All the forms of electromagnetic radiation form the electromagneticspectrum

  3. Wave Features • Wavelength (λ): The distance between corresponding points on adjacent waves • Units are metric units of length. Commonly nm.

  4. Wave Features • Frequency (ν): The number of waves that pass a given point in a specific time. • Unit = Hertz (Hz) = 1/s = s-1

  5. Calculations Wavelength c=λν Frequency Speed of light Rearrange to solve for frequency and wavelength: c c ν = λ = ν λ

  6. Example Calculation • Problem: • Given the speed of light = 3.0 x 108 m/s, calculate the wavelength of the electromagnetic radiation whose frequency is 7.500 x 1012 Hz. • Solution: c 3.0 x 108m/s λ = = = 4.0 x 10-5m ν 7.500 x 1012Hz

  7. Max Plank • Found that there is a direct relationship between energy and frequency. • Plank’s constant • h = 6.626 x 10-34 J· s E = hν Plank’s Constant Energy frequency

  8. Line Emission Spectra • A series of specific wavelengths of emitted light created when the visible portion of light from excited atoms is shined through a prism.

  9. Visible Spectrum ROY G BIV

  10. Atoms and Their Energy • Ground State: The lowest energy state of an atom • Excited State: A state in which an atom has a higher energy than it has in its ground state

  11. Atoms and Their Energy • When an excited atom returns to its ground state, it gives off energy it gained in the form of electromagnetic radiation.

  12. Hydrogen Line Spectrum • When the visible portion of the emitted light is passed through a prism, it is separated into specific wavelengths.

  13. Bohr Model • Based on the wavelengths of hydrogen’s line emission spectrum, Bohr calculated the energies that an electron would have in the energy levels for a hydrogen atom.

  14. Bohr Model Calculations • The energy of each photon is calculated by subtracting the energy of the ground state from the energy of the excited state. • These energies correspond to specific wavelengths of the electromagnetic spectrum.

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