Identify the false statement about atomic and ionic radii. (LO 6.3) (a) I- has a larger radius than Br- (b) Ba2+ has a smaller radius than Ba (c) Te has a larger radius than Te2- (d) Sr2+ has a smaller radius than Se2-

Verified step by step guidance

1. Step 1: Understand the concept of atomic and ionic radii. Atomic radius refers to the size of a neutral atom, while ionic radius refers to the size of an ion. When an atom gains electrons to form an anion, its radius typically increases due to increased electron-electron repulsion. Conversely, when an atom loses electrons to form a cation, its radius typically decreases due to reduced electron-electron repulsion.
2. Step 2: Analyze statement (a): I- has a larger radius than Br-. Compare the ionic radii of I- and Br-. Both are anions, and I- is located below Br- in the periodic table, which generally means it has a larger radius due to the addition of an electron shell.
3. Step 3: Analyze statement (b): Ba2+ has a smaller radius than Ba. Compare the ionic radius of Ba2+ with the atomic radius of Ba. Ba2+ is a cation formed by losing two electrons, which typically results in a smaller radius compared to the neutral atom.
4. Step 4: Analyze statement (c): Te has a larger radius than Te2-. Compare the atomic radius of Te with the ionic radius of Te2-. Te2- is an anion formed by gaining two electrons, which typically results in a larger radius compared to the neutral atom. This statement seems incorrect based on the general trend.
5. Step 5: Analyze statement (d): Sr2+ has a smaller radius than Se2-. Compare the ionic radius of Sr2+ with the ionic radius of Se2-. Sr2+ is a cation, and Se2- is an anion. Generally, cations have smaller radii than anions, especially when comparing ions from different groups.