The first ionization energy of a carbon atom is 1.81 aJ. What is the frequency and wavelength, in nanometers, of photons capable of just ionizing carbon atoms?


lambda =_____nm

Assuming an ionization efficiency of 47.0%, how many such photons are needed to ionize 1.00 × 1016 atoms?


  1. 👍 0
  2. 👎 0
  3. 👁 1,064
  1. What's 1.81 aJ? Do you mean kJ so IP = 1810 J.
    Then 1810 = hc/wavelength. Solve for wavelength in meters and convert to nm.
    c = freq x wavelength will let you solve for freq.

    1810 J/atom x 1E16 atoms x 0.47 = ?

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