What is the solubility of hydroxides?

The hydroxides of sodium, potassium, and ammonium are very soluble in water. The hydroxides of calcium and barium are moderately soluble. The oxides and hydroxides of all other metals are insoluble.

Why does the thermal stability of hydroxides increase down the group?

In the periodic table, as we go down in the group the lattice enthalpy increases, which leads to an increase in thermal stability of the hydroxide.

Why does the solubility of alkaline earth metal hydroxides in water increase down the group?

Among alkaline earth metal hydroxides, the anion being common, the cationic radius will influence the lattice enthalpy. Since lattice enthalpy decreases much more than the hydration enthalpy with increasing ionic size, the solubility increases down the group (↓).

Why some hydroxides are insoluble in water?

The insolubility of the hydroxides of the transition metals can be explained both by the increasingly large ionization energies that result from successively removing electrons (or negatively charged hydroxide molecules in this case) from the metal cation, and the greater effective nuclear charge on the electrons …

What is the trend of solubility in group 2?

Group II metal hydroxides become more soluble in water as you go down the column. This trend can be explained by the decrease in the lattice energy of the hydroxide salt and by the increase in the coordination number of the metal ion as you go down the column.

Does thermal stability of hydroxides of alkaline earth metals decrease down the group?

Explanation: Stability of ionic compounds decreases with decrease in lattice enthalpy. Thus stability of alkaline earth metal hydroxides decreases with decrease in lattice enthalpy as the size of alkali earth metal cations increases down the group.

Why does solubility of Group 2 hydroxides increase while progressing down the group?

The hydration enthalpy also decreases since the size of the cation increases. However, due to the square factor, the lattice enthalpy decreases faster than the hydration enthalpy. This is why the solubility of Group 2 hydroxides increases while progressing down the group. Now let’s look at $\\ce{SO4^2-}$.

What is the relationship between enthalpy of solution and solubility?

The relationship between enthalpy of solution and solubility. The assumption is made that the more endothermic (or less exothermic) the enthalpy of solution is, the less soluble the compound. So sulphates and carbonates become less soluble as you go down the Group; hydroxides become more soluble.

How does hydroxide interact with water?

Hydroxide interacts well with water, but the smaller Group 2 cations can compete successfully with water for hydroxide ions; the larger cations can’t. (On the other hand, water doesn’t solvate the big cations as well, either.)

What happens to lattice enthalpy as you go down Group 2?

While progressing down Group 2, the size of the cation increases since the number of shells increases to accommodate to the extra electrons. Due to this, the distance between the centres of mass of the cation and the anion increases and by definition, the lattice enthalpy decreases.