Chemical Forums

Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: xshadow on December 02, 2020, 06:01:34 AM

Title: electron affinity: halide
Post by: xshadow on December 02, 2020, 06:01:34 AM

I know that the electron affinity trend for halide is:

F > Cl > Br > I

So Cl has a higher electron affinity than Br  ....in other words  Cl^- is more stable than Br^- cause the higher value of electron affinity

Now my doubts is that I always knew that Br^- is  more stable than Cl^- (the opposite of what  I said when I thought at electron affinity) because the negative charge is "delocalized" on a bigger volume


So I get two opposite conclusions if I think at the charge delocalization or at the electron affinity....
Is this difference attributable at gas phase vs "liquid" phase?? why?

Thanks