The ionic radii of and are experimentally found to be and respectively. Using the arithmetic mean as — Periodic Table and Periodicity Chemistry Question
Question
The ionic radii of $S^{2-}$ and $Te^{2-}$ are experimentally found to be $1.84 \text{ \AA}$ and $2.20 \text{ \AA}$ respectively. Using the arithmetic mean as a rough approximation, what is the predicted ionic radius of $Se^{2-}$ in $\text{\AA}$?
Answer: 2.02
💡 Solution & Explanation
Selenium ($Se$) is located exactly between Sulphur ($S$) and Tellurium ($Te$) in Group 16 of the periodic table. By interpolating the radii as an arithmetic mean: predicted radius $= \frac{1.84 + 2.20}{2} = \frac{4.04}{2} = 2.02 \text{ \AA}$.
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