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(D) The melting point $(MP)$ of an ionic crystal is directly proportional to its lattice energy.Lattice energy is inversely proportional to the intern

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the internuclear distance $(r^+ + r^-)$ is greater for $RbBr$ than for $NaF$

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(D) The melting point $(MP)$ of an ionic crystal is directly proportional to its lattice energy.Lattice energy is inversely proportional to the internuclear distance $(r^+ + r^-)$ between the ions.Since $Na^+$ and $F^-$ are smaller ions compared to $Rb^+$ and $Br^-$,the internuclear distance $(r^+ + r^-)$ is significantly smaller for $NaF$ than for $RbBr$.Therefore,$NaF$ has a much higher lattice energy and a higher melting point compared to $RbBr$.

The principal reason that the melting point of $NaF$ is much higher than that of $RbBr$ is that

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