Answer :
Final answer:
The atomic radius of a Chlorine atom likely falls between Fluorine and Bromine. Given that, a sensible estimate would be 89 pm.
Explanation:
The atomic radii of elements generally increase as you move down a group in the periodic table. This is because additional electrons are added in outer shells, leading to an increase in size. From the given atomic radii of F (Fluorine), Br (Bromine), and I (Iodine), we observe that the atomic radii increase from Fluorine to Bromine to Iodine as we move down the group.
Since Chlorine (Cl) lies between F and Br in the periodic table, we can reasonably estimate that its atomic radius should be between 64 pm (F) and 114 pm (Br). The only choice within this range is b. 89 pm. This is a reasonable estimate for the atomic radius of Chlorine.
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