This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Here's the explanation for question (ii): (ii) MgCl_2 exists in the hydrated form while NaCl does not. Step 1: Compare the charge density of Mg^2+ and Na^+ ions. The Mg^2+ ion has a smaller ionic radius and a higher charge (+2) compared to the Na^+ ion, which has a larger ionic radius and a lower charge (+1). This gives Mg^2+ a significantly higher charge density than Na^+. Step 2: Explain the effect of high charge density on hydration. Due to its high charge density, the Mg^2+ ion has a strong electrostatic attraction for the lone pairs of electrons on the oxygen atom of water molecules. This strong attraction allows Mg^2+ to effectively polarize water molecules and form strong coordinate bonds, leading to the formation of stable hydrated ions. Step 3: Conclude why MgCl_2 is hydrated and NaCl is not. The Na^+ ion, with its lower charge density, does not attract water molecules strongly enough to form stable hydrated complexes. Therefore, MgCl_2 readily forms hydrates (e.g., MgCl_2 · 6H_2O), while NaCl typically exists in its anhydrous form. Drop the next question!