The correct order regarding the solubility of alkaline carth...

The correct order regarding the solubility of alkaline carth metal halide in water is (1) $\mathrm{BeCl}_{2}>\mathrm{MgCl}_{2}>\mathrm{CaCl}_{2}>\mathrm{SrCl}_{2}>\mathrm{BaC} \mathrm{l}_{2}$ (2) $\mathrm{MgCl}_{2}>\mathrm{CaCl}_{2}>\mathrm{BeCl}_{2}>\mathrm{BaCl}_{2}>\mathrm{SrCl}_{2}$ (3) $\mathrm{BaCl}_{2}>\mathrm{MgCl}_{2}>\mathrm{CaCl}_{2}>\mathrm{BeCl}_{2}>\mathrm{SrCl}_{2}$ (4) $\mathrm{CaCl}_{2}>\mathrm{MgCl}_{2}>\mathrm{SrCl}_{2}>\mathrm{BaCl}_{2}>\mathrm{BeCl}_{2}$

The correct order regarding the solubility of alkaline carth metal halide in water is
(1) $\mathrm{BeCl}_{2}>\mathrm{MgCl}_{2}>\mathrm{CaCl}_{2}>\mathrm{SrCl}_{2}>\mathrm{BaC} \mathrm{l}_{2}$
(2) $\mathrm{MgCl}_{2}>\mathrm{CaCl}_{2}>\mathrm{BeCl}_{2}>\mathrm{BaCl}_{2}>\mathrm{SrCl}_{2}$
(3) $\mathrm{BaCl}_{2}>\mathrm{MgCl}_{2}>\mathrm{CaCl}_{2}>\mathrm{BeCl}_{2}>\mathrm{SrCl}_{2}$
(4) $\mathrm{CaCl}_{2}>\mathrm{MgCl}_{2}>\mathrm{SrCl}_{2}>\mathrm{BaCl}_{2}>\mathrm{BeCl}_{2}$

Key Concepts

Alkaline Earth Metal Halides

This concept refers to salts formed between the alkaline earth metals (Group 2 elements) and halide ions. Their properties, including solubility in water, are significantly influenced by the size, charge density, and the nature of the bonding between the metal cation and the halide anion.

Solubility Trends

Solubility trends in ionic compounds are determined by the interplay between lattice energy and hydration energy. In the context of alkaline earth metal halides, the overall solubility in water results from the balance between the energy needed to break the ionic lattice and the energy released upon hydration of the ions.

Lattice Energy

Lattice energy is the energy released when ions come together to form a crystalline lattice. It depends on the charge and size of the ions; smaller and highly charged ions yield higher lattice energies. In alkaline earth metal halides, variations in lattice energy, influenced by ionic sizes, directly affect their solubility.

Hydration Enthalpy

Hydration enthalpy is the energy released when ions interact with water molecules. In metal halides, higher hydration enthalpy helps to overcome lattice energy, increasing solubility. The effectiveness of hydration is largely dependent on the size and charge density of the metal ions.

Ionic Size and Polarization Effects

Ionic size and polarization play a crucial role in determining how well a salt dissolves in water. Smaller, more polarizing cations can distort the electron cloud of the halide ion, leading to partial covalency which affects both lattice and hydration energies. This is particularly important for metals like beryllium, where pronounced polarization leads to anomalous solubility behavior.

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