(Solved):   Use the values below to calculate the lattice of enthalpy of \( \mathrm{CaCl}_{2} \). Latt ...

 

Use the values below to calculate the lattice of enthalpy of \( \mathrm{CaCl}_{2} \). Lattice energy \( \mathrm{CaCl}^{2+} \mathrm{Ca}^{2+}(\mathrm{g})+2 \mathrm{Cl}(\mathrm{g}) \rightarrow \mathrm{CaCl}_{2}(\mathrm{~s}) \) B. Use the Kapustinskii equation to estimate the lattice energy for \( \mathrm{CaCl}_{2} \) Given that radius \( \mathrm{Ca}^{2+}=100 \mathrm{pm} \), radius \( \mathrm{Cl}^{-}=181 \mathrm{pm} \), and \( \mathrm{k}=107,900 \mathrm{pmkJmol}^{-1} \) \[ \Delta_{\text {latt }} U= \] C. Based on the results obtained assumptions made about \( \mathrm{CaCl}_{2} \) being ionic are These results indicate that \( \mathrm{CaCl}_{2} \) solid has a amount of covalent character.