* Atomic Size: Bromine is larger than fluorine in terms of atomic size because it has more electron shells.
* Ionic Charge: Both bromine and fluorine gain one electron to form their respective anions (Br- and F-).
* Effective Nuclear Charge: Bromine has a larger number of protons in its nucleus than fluorine, which creates a stronger attraction between the nucleus and its electrons. This stronger attraction pulls the electrons closer to the nucleus, making the ionic radius of bromine smaller than fluorine's.
In summary: Although bromine is larger than fluorine as an atom, its higher effective nuclear charge results in a smaller ionic radius.
