6.1 Physical Properties

2.1 Physical Properties
2.2 Chemical properties

6.1 Physical Properties
6.2 Chemical Properties

1. Atomic and ionic radii: Both are smaller than corresponding members of alkali metals.

2. Ionisation energy: Due to the large size of alkaline earth metals, they have fairly low values of ionization energies as compared to the p-block elements. Along the group ionization energy decreases as the atomic number increases.

Note: Because their IE is larger than that of their alkali metal neighbours, the group $2$ metals are less reactive than alkali metals. The general reactivity trend is $$Ba>Sr>Ca>Mg>Be$$

3. Electropositive or metallic character: Alkaline earth metals are highly electropositive i.e., metallic character increases down the group. However they are less electropositive than alkali metals.

4. Melting and boiling point: They have high melting and boiling points as compared to those of alkali metals due to their small size and close packing.

5. Heat of hydration: Heat of hydration of $M^{2+}$ decreases with an increase in their ionic size and their values are greater than that of alkali metal ions.

6. Reducing character: They are weaker reducing agents than alkali metals. But reducing character increases down the group because they have greater tendency to lose electrons, so they act as good reducing agents.