Provide an example of the reactivity and solubility of Group 2 elements.

Group 2 elements are reactive and have varying solubility in water.

Group 2 elements, also known as alkaline earth metals, are highly reactive due to their low ionization energies. They readily lose their two valence electrons to form 2+ cations, which makes them highly reactive with non-metals such as oxygen, chlorine, and sulfur. For example, magnesium reacts with oxygen to form magnesium oxide, which is a white powder commonly used in medicine and as a refractory material.

In terms of solubility, Group 2 elements have varying degrees of solubility in water. Beryllium and magnesium are relatively insoluble in water, while calcium, strontium, and barium are more soluble. This is due to the increasing size of the atoms down the group, which leads to a decrease in the lattice energy and an increase in the hydration energy. As a result, the larger atoms are more likely to dissolve in water and form hydrated ions.

The reactivity and solubility of Group 2 elements have important applications in various industries. For example, calcium and magnesium are commonly used in the production of alloys, while barium is used in the production of glass and ceramics. The reactivity of these elements also makes them useful in the production of fireworks and flares, as well as in the treatment of wastewater and soil. Overall, the properties of Group 2 elements make them important components of many materials and processes.