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Question

State whether the following statements are true or false.
S1 : AgI is less soluble in water than AgF due to more polarization of I− in comparison to F− ion.
S2 : The melting point of BaCl2 is higher than the melting point of BeCl2 due to greater ionic nature of BaCl2.
S3 : The order of hydrated radii is : Al3+(aq)>Mg2+(aq)>Na+(aq)

A
T T T
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B
T T F
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C
T F T
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D
F T T
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Solution

The correct option is A T T T
S1 : 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.

S2 : Ba2+ ion has low charge density due to its larger size when compared to Be2+ ion. Hence it has a low polarizing power when compared to Be2+. So, according to Fajan's rule, BaCl2 has a higher ionic character and thus has a higher melting point.

S3 : Higher the charge density, larger will be the hydrated radii.
Order of charge density : Al3+>Mg2+>Na+
Hence, the order of hydrated radii will follow the same order i.e. Al3+(aq)>Mg2+(aq)>Na+(aq)

Thus, all the three statements are correct.

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