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?