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Given the ionic radii Na+ = 0.095 nm, Cl− = 0.181 nm, Zn2+ = 0.074 nm, S2− = 0.184 nm, Ti4+ = 0.068 nm, O2− = 0.140 nm, and Cs+ = 0.169 nm, identify the correct statement(s) using the radius-ratio criterion.

1. Na+ ions occupy octahedral voids formed between close-packed layers of Cl− ions.
2. Zn2+ ions occupy tetrahedral voids.
3. Cs+ ions are arranged in a simple cubic lattice of Cl− ions.
4. All of the above.

Correct answer: All of the above.

Solution

All the statements are correct based on the radius-ratio criterion, which helps determine the coordination number and arrangement of ions in a crystal lattice. Na+ fits well in octahedral voids due to its size relative to Cl−, Zn2+ is small enough to occupy tetrahedral voids, and Cs+ can be arranged in a simple cubic lattice with Cl− due to its larger ionic radius.

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