If the ionic character of Na^{+} and S^{2-} i | vedclass

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(A) According to Fajan's rule,the solubility of an ionic compound in water is inversely proportional to its covalent character.Covalent character incr

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$MgS$

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(A) According to Fajan's rule,the solubility of an ionic compound in water is inversely proportional to its covalent character.Covalent character increases with higher charge density and smaller size of the cation (polarizing power) and larger size of the anion (polarizability).Comparing the given compounds,$MgS$ consists of $Mg^{2+}$ and $S^{2-}$ ions. Both ions have high charges,and $S^{2-}$ is a large anion,which leads to significant covalent character.Compounds with higher covalent character are generally less soluble in polar solvents like water.Therefore,$MgS$ is the least soluble among the given options.

If the ionic character of $Na^{+}$ and $S^{2-}$ ions is greater than that of $Mg^{2+}$ and $Cl^{-}$ ions,which of the following will be the least soluble in water?

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