Lithium fluoride (LiF) and cesium fluoride (CsF) each contain singly charged ions
CHEMISTRY · Subjective · CBSE · Chemistry · Chemical Bonding and Molecular Structure · Chemical Bonding and Molecular Structure
Problem
Lithium fluoride (LiF) and cesium fluoride (CsF) each contain singly charged ions. The ionic radii are Li⁺ = 76 pm, Cs⁺ = 167 pm, and F⁻ = 133 pm. Using the sum of the cation and anion radii as the center-to-center distance, determine which compound is predicted to have the more exothermic lattice energy and state the approximate factor by which its magnitude differs from the other compound.