Using the trends in the periodic table, rank the following atoms in order of increasing electronegativity. Br, F, I
In general, electronegativity increases as you move from left to right across a period on the periodic table and decreases as you move down a group. Based on this trend, we can rank the atoms Br, F, and I in order of increasing electronegativity:
I < Br < F
Iodine (I) has the lowest electronegativity because it is located at the bottom of Group 17 (halogens) and is further away from the nucleus. Bromine (Br) has a slightly higher electronegativity than iodine because it is closer to the nucleus. Finally, fluorine (F) has the highest electronegativity among these three elements because it is the furthest to the right on the periodic table and the closest to the nucleus.