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Electron affinities

  1. Aug 24, 2014 #1

    kay

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    Why is the EA of Fluorine higher than chlorine when it shouldn't be according to periodic trends?

    And in general when it is easy to add an electron to a substance, then is the EA high or low?
     
  2. jcsd
  3. Aug 29, 2014 #2

    Greg Bernhardt

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    Staff: Admin

    I'm sorry you are not finding help at the moment. Is there any additional information you can share with us?
     
  4. Aug 29, 2014 #3

    kay

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    I forgot to add that by EA i meant 'Electron Affinity.' I think that's all. :(
     
  5. Aug 30, 2014 #4
    Are you referring to electronegativity? The trend is higher as you go up and right on the periodic table, so F being more electronegative than Cl does not defy the trend.

    [​IMG]
     
  6. Aug 31, 2014 #5

    kay

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    I mean Electron Gain Enthalpy or Electron Affinity.
     
  7. Aug 31, 2014 #6

    kay

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    So is there no one who knows the answer? :eek:
     
  8. Aug 31, 2014 #7
  9. Aug 31, 2014 #8
    I think it can be explained by use of electron configuration of both F- and Cl-; one is more stable than the other. Therefore the energy to remove an electron from it is essentially larger than that of the other.
     
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