The solubility order for alkali metal fluoride in water is (a) LiF<RbF<KF<NaF (b) RbF<KF<NaF<LiF

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The solubility order for alkali metal fluoride in water is...

The solubility order for alkali metal fluoride in water is (a) $\mathrm{LiF}<\mathrm{RbF}<\mathrm{KF}<\mathrm{NaF}$ (b) $\mathrm{RbF}<\mathrm{KF}<\mathrm{NaF}<\mathrm{LiF}$ (c) $\mathrm{LiF}>\mathrm{NaF}>\mathrm{KF}>\mathrm{RbF}$ (d) $\mathrm{LiF}<\mathrm{NaF}<\mathrm{KF} \leq \mathrm{RbF}$

The solubility order for alkali metal fluoride in water is
(a) $\mathrm{LiF}<\mathrm{RbF}<\mathrm{KF}<\mathrm{NaF}$
(b) $\mathrm{RbF}<\mathrm{KF}<\mathrm{NaF}<\mathrm{LiF}$
(c) $\mathrm{LiF}>\mathrm{NaF}>\mathrm{KF}>\mathrm{RbF}$
(d) $\mathrm{LiF}<\mathrm{NaF}<\mathrm{KF} \leq \mathrm{RbF}$

Key Concepts

Hydration Energy

Hydration energy is the energy released when water molecules surround and interact with dissolved ions. This energy stabilizes the ions in solution, and if the hydration energy is high enough, it can overcome the lattice energy, thereby enhancing the solubility of the ionic compound.

Ionic Radius and Periodic Trends

Ionic radius is the measure of the size of an ion, and it significantly affects both lattice and hydration energies. In the context of alkali metal compounds, as the ionic radius increases down the group, the lattice energies tend to decrease due to the larger distance between ion centers, while the hydration energies typically decrease due to less effective charge stabilization. These opposing trends help determine the overall solubility behavior of the salts.

Ionic Solubility

Ionic solubility refers to the tendency of an ionic compound to dissolve in a solvent such as water. This process is governed by the balance between the energy required to break the ionic lattice and the energy released when the individual ions become hydrated by water molecules.

Lattice Energy

Lattice energy is the energy released when oppositely charged ions come together to form a solid crystal lattice. It is a measure of the bond strength in an ionic compound; higher lattice energies indicate stronger ionic bonds, which can reduce solubility because more energy is needed to break apart the lattice during dissolution.

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