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Ionization energy of hydrogen

  1. May 19, 2009 #1
    1. The problem statement, all variables and given/known data
    Estimate the energy of an electron in a hydrogen atom and hence deduce an approximate formula for the ionization energy of hydrogen. How accurate is your formula?


    2. Relevant equations
    Don't know but it is in the field of quantum mechanics


    3. The attempt at a solution

    Ionisation Energy is energy required to remove an electron.

    Electrostatic Potential (energy per unit charge) V=q/(4πε_0 r)= e/(4πε_0 r)

    For a Bohr atom (Z=1), energy required to remove an electron from the atom with a nucleus of charge e and a radius r0 is the Electrostatic Potential Energy:

    PE=qV = e^2/(4πε_0 r)×1/e
    =(1.6×10^(-19))/(4π×8.85×10^(-12)×10^(-15) )
    =1.4MeV

    The equation estimates the distance of the electron from the proton in the nucleus as a precise value – this is not the case. An electron’s position is given by a wave-function probability density and it is in effect occupying the whole of the atom at once.

    IS ANY OF THIS RIGHT???
     
  2. jcsd
  3. May 19, 2009 #2

    Matterwave

    User Avatar
    Science Advisor
    Gold Member

    1.4MeV is about 100,000 times too large.

    I think it's because your radius appears to be 100,000 times too small.

    You are right that this semi-classical model of the electron is wrong, but you can get a good estimate of the ionization energy using this. And I think that's what the question asks.
     
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