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Electromagnetic Waves

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Electromagnetic Waves A wave transmits energy from the source to the receiver. Electromagnetic waves do this by disturbing the electric and magnetic fields ... – PowerPoint PPT presentation

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Date added: 23 July 2020
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Title: Electromagnetic Waves


1
Electromagnetic Waves
  • A wave transmits energy from the source to the
    receiver.
  • Electromagnetic waves do this by disturbing the
    electric and magnetic fields surrounding the
    earth.
  • The types of electromagnetic waves are arranged
    on a spectrum from greatest to smallest frequency.

2
Electromagnetic Spectrum
3
Electromagnetic Spectrum
4
Wave Properties
  • Wavelength (?) is the distance between two
    successive waves.
  • Frequency (f) is the number of waves passing a
    point per second.
  • V f ? wave speed equation
  • Wave speed (v) is the speed of electromagnetic
    waves. In a vacuum this is 3.0 x 108 m/s or
    186,000 miles per second!

5
Wave Properties
6
Bohr Model of the Atom
  • To explain the emission of light, Bohr came up
    with a radical model of the atom which had
    electrons orbiting around a nucleus.
  • This similarity between a planetary model and the
    Bohr Model of the atom ultimately arises because
    the attractive gravitational force in a solar
    system and the attractive Coulomb (electrical)
    force between the positively charged nucleus and
    the negatively charged electrons in an atom are
    mathematically of the same form.

7
Energy Levels of the Atom
  • In the Bohr model, electrons can jump to higher
    energy states by the addition of energy of
    certain frequencies
  • The excited electron is unstable and falls down
    to ground state giving off electromagnetic energy
    equal in frequency to the energy change.

8
Hydrogen Emission Series
  • The electrons can move to only certain locations
    from the nucleus
  • The result of this restriction in movement is
    specific and distinct wavelengths of EM radiation
    is given off as the electrons transition.

9
Energy Quantified
  • The energy transitions are quantified and thus
    the transitions accept and release only certain
    energies of E/M radiation.
  • The energy of each level for the hydrogen atom is
    given by the equation
  • En RH/n2
  • RH is called the Rydberg constant
  • RH 2.180 x 10-18 J

10
Energy to Wavelength
  • E h f
  • h is a constant in nature
  • h 6.626 x 10-34 J/Hz
  • Rearranging the frequency of absorbed or emitted
    light is
  • f E h

11
Atomic Spectra
  • White light emits all colors because a multitude
    of electron transitions occur between energy
    levels.
  • Spectral Lines give evidence of electron
    transitions.
  • A specific species of gas emits only a limited
    amount of spectral colors because of a more
    limited availability of electron transitions.

12
Emission Spectra for H2 and He
13
More Emission Spectra Na, Ne, Hg
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