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Quantization/hydrogen atom problem

  1. Nov 17, 2005 #1
    I have a homework problem that goes like this.
    A beam of electrons is incident upon a gas of hydrogen atoms. What minimum speed must the electrons have to cause the emission of 656 nm light from the 3 -> 2 transition of hydrogen?
    So I had a couple of thoughts
    1) It was the velocity needed to have state 3 orbit, but that's not right.
    2) It was the velocity needed to have n=2 orbit, but that's not right either.
    3) It was the velocity such that an electron had KE equal to the difference in E of states 3 and 2 but that's not it either.
    I suppose the wavelength of the light has something to do with this but it's just the wavelength of hydrogen emission 3->2 so I dunno what that tells you.
  2. jcsd
  3. Nov 17, 2005 #2


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    Staff: Mentor

    In order to produce transitions from n=3 to n=2 , you have to get the atoms into the n=3 state to begin with. Atoms are normally in their ground state (n=1).
  4. Nov 18, 2005 #3
    So if the incoming electrons had KE greater than the ionization energy it could remove an electron from the n=1 orbit and the atom completely. So a KE equal to the difference of the n=1 E and n=3 E would move it to the n=3 orbit? Then the orbiting electron simply falls back to the n=2 level?
    *goes to try it*

    It works!
    Danke sehr
    Does it just go back to n=2 because it's attacted to the nucleus or?
    Last edited: Nov 18, 2005
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