Why does fluorine have higher electron affinity than chlorine?

[kay]

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?

 

[Greg Bernhardt]

I'm sorry you are not finding help at the moment. Is there any additional information you can share with us?

 

[kay]

I forgot to add that by EA i meant 'Electron Affinity.' I think that's all. :(

 

[aroc91]

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.

 

[kay]

I mean Electron Gain Enthalpy or Electron Affinity.

 

[kay]

So is there no one who knows the answer?

 

[Yanick]

I think you will find this website (http://chemwiki.ucdavis.edu/Physica...ic_and_Molecular_Properties/Electron_Affinity) discussed exactly the issue you are asking about.

 

[Medicol]

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.