Solubilities (other things also included)

ALKALI METALS (specially for anand)
(IIT syll: Oxides, peroxides, hydroxides, carbonates, bicarbonates, chlorides and sulphates of sodium, potassium, magnesium and calcium)

Alkali and alkaline earth metal hydroxides

Solubility increases down the group as ionic nature of the hydroxides increase

Alkaline earth metal sulphates:

Solubility decreases down the group

Alkali metal sulphates

Solubility increases down the group

Stability of hydrides (alkali and alkaline earth metal)

*Thermal stability decreases down the group (as covalent nature decreases)
*Reducing character increases down the group. (as stability decreases)

Halides of alkaline earth metals
*The solubility of the halide decreases on descending the group because the hydration enthalpies decrease faster than the lattice enthalpies do.
*The solubilities of the fluorides of group 2 follow the opposite trend however. This is because the very small size of the fluoride ions means that in the solid state the much larger M2+ ions are more and more in contact with each other as their size increases causing a faster lowering of the lattice energies.

Carbonates/bicarbonates of alkaline earth metals
The carbonates of the metals, MCO₃, are all largely insoluble and the solubility decreases on going down the group.

Carbonates/bicarbonates of alkali metals
The solubilities of carbonates and bicarbonates of alkali metals increase as we go down the group from lithium to caesium.