General Properties:

* Location on the Periodic Table: Group 2, second column from the left.

* Metallic Properties: They are all shiny, silvery-white, and highly reactive metals.

* Electropositivity: They have a strong tendency to lose two electrons to form cations with a +2 charge. This makes them highly reactive.

* Reactivity: They are more reactive than alkali metals but less reactive than the transition metals.

* Reducing Agents: Due to their strong tendency to lose electrons, they act as strong reducing agents in chemical reactions.

Specific Properties:

* Melting and Boiling Points: Have relatively high melting and boiling points, increasing down the group.

* Density: Have moderate densities, increasing down the group.

* Hardness: They are relatively soft metals.

* Electrical Conductivity: Good conductors of electricity.

* Thermal Conductivity: Good conductors of heat.

Reactions:

* Reaction with Water: Reacts readily with water, producing hydrogen gas and the corresponding metal hydroxide. The reaction becomes more vigorous as you go down the group.

* Reaction with Oxygen: Reacts with oxygen to form oxides, and some form peroxides.

* Reaction with Acids: Reacts vigorously with acids to form salts and hydrogen gas.

Uses:

* Calcium: Used in construction materials (cement, mortar), as a reducing agent in metallurgy, and in making alloys.

* Magnesium: Used in lightweight alloys, in fireworks, and in the production of magnesium oxide, a refractory material.

* Barium: Used in pyrotechnics, in x-ray imaging, and as a component in barium sulfate, which is used in medical imaging.

Examples of Alkaline Earth Metals:

* Beryllium (Be)

* Magnesium (Mg)

* Calcium (Ca)

* Strontium (Sr)

* Barium (Ba)

* Radium (Ra)

Important Note: The reactivity of alkaline earth metals increases as you move down the group. This is due to the increase in atomic radius and the decrease in ionization energy.