Question

State whether the following statements are true or false.
$S_1$ : $AgI$ is less soluble in water than $AgF$ due to more polarization of $I^{-}$ in comparison to $F^{-}$ ion.
$S_2$ : The melting point of $BaC{l}_2$ is higher than the melting point of $BeC{l}_2$ due to greater ionic nature of $BaC{l}_2$.
$S_3$ : The order of hydrated radii is : $A{l}^{3+}\left(aq\right)>M{g}^{2+}\left(aq\right)>N{a}^{+}\left(aq\right)$

• A. T T T
• B. T T F
• C. T F T
• D. F T T

Answer 1

The correct option is A T T T

$S_1$ : According to Fajan's rule, polarizability of $I^{-}$ in $AgI$ is higher than that of $F^{-}$ in $AgF$. Hence $AgI$ is less soluble than $AgF$, due to its high covalent nature.

$S_2$ : $B{a}^{2+}$ ion has low charge density due to its larger size when compared to $B{e}^{2+}$ ion. Hence it has a low polarizing power when compared to $B{e}^{2+}$. So, according to Fajan's rule, $BaC{l}_2$ has a higher ionic character and thus has a higher melting point.

$S_3$ : Higher the charge density, larger will be the hydrated radii.
Order of charge density : $A{l}^{3+}>M{g}^{2+}>N{a}^{+}$
Hence, the order of hydrated radii will follow the same order i.e. $A{l}^{3+}\left(aq\right)>M{g}^{2+}\left(aq\right)>N{a}^{+}\left(aq\right)$

Thus, all the three statements are correct.