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How close must the wavelength of a photon be for an atom to absorb it?

  1. Jun 30, 2012 #1
    When a photon has a wavelength close to the energy needed for an electron jump in an atom, the atom will absorb the photon. How close must the wavelength be to the energy required for the atom to still absorb it?
     
  2. jcsd
  3. Jul 1, 2012 #2
    Other members correct me if am wrong but I believe most photon energies are absorbed the electron. Most times the photon has not enough energy to excite the electron to an upper energy level, so the electron does not move and absolves the light.
    If the photon has equal or more energy than the energy difference of the electron cloud orbitals the electron is excited up where it imminently comes back down and remit the photon.
     
  4. Jul 1, 2012 #3
    Exact, photons arise from complementary quantization phenomena
     
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