Explain why the lattice energy of CaSe is approximately 4 times as large as that of KBr. Check all that apply. Check all that ap
ply. According to Coulomb’s law, the Ca and Se ions have 4 times the attractive force (2+ × 2-) than that of the K and Br ions (1+ × 1-). According to Coulomb’s law, the Ca and Se ions have 4 times the repulsive force (2+ × 2-) than that of the K and Br ions (1+ × 1-). The lattice energy depends only on the sizes of constituent ions of the compound. The Ca2+ and K+ ions are four times larger in size than the Se2- and Br- ions. They Ca2+ and K+ ions are similar in size, as are the Se2- and Br- ions. Thus, the major difference in the lattice energies for these two compounds is due to the difference in the magnitude of the ionic charge on each ion. The lattice energy depends on the sizes of constituent ions of the compound. The Ca2+ is four times larger in size than the Se2- ion.
According to Coulomb’s law, the Ca and Se ions have 4 times the attractive force (2+ × 2-) than that of the K and Br ions (1+ × 1-).
Explanation:
From Coulomb's law, the attractive force between calcium and selenium ions is four times the attractive force between potassium and bromide ions.
This has something to do with size and magnitude of charge. Calcium ions and selenide ions are smaller and both carry greater charge magnitude than potassium and bromide ions. This paves way for greater electrostatic attraction between them when the distance of the charges apart is minimal. Hence a greater lattice energy.
<span>The lattice structure in a metal is weaker than the lattice structure of an ionic compound. This is because the metals have free electrons which can freely move around while ionic compounds are strongly bonded. Hope this answers the question.</span>
