Write a balanced equation that predicts the reaction of rubidium (Rb) with (a) \(\mathrm{H}_{2} \mathrm{O}(l)\) (b) \(\mathrm{Cl}_{2}(g)\) (c) \(\mathrm{H}_{2}(g)\)

Understanding the behavior of rubidium (Rb), an alkali metal, in chemical reactions is essential for students studying chemistry. Rubidium is highly reactive and typically undergoes rapid and vigorous reactions. One such example is its reaction with water. When rubidium comes into contact with water, it reacts to form rubidium hydroxide and hydrogen gas. This reaction can be represented by the equation:
\[2\mathrm{Rb(s)} + 2\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2\mathrm{RbOH}(aq) + \mathrm{H}_{2}(g)\].
Another common reaction is when rubidium reacts with chlorine gas to form rubidium chloride, a type of salt. This synthesis reaction is outlined by:
\[2\mathrm{Rb(s)} + \mathrm{Cl}_{2}(g) \longrightarrow 2\mathrm{RbCl}(s)\].
Lastly, rubidium can also react with hydrogen gas to produce rubidium hydride, as shown:
\[2\mathrm{Rb(s)} + \mathrm{H}_{2}(g) \longrightarrow 2\mathrm{RbH}(s)\].
In each of these examples, stoichiometry—a cornerstone concept in chemistry involving the quantitative relationship between reactants and products in a chemical reaction—is used to balance the chemical equations, ensuring that the number of atoms for each element is equal on both sides.

Alkali metals are placed in group 1 of the periodic table and are known for their high reactivity rates due to their single valence electron. This makes them eager to react and form more stable compounds. The reactivity increases as you move down the group, meaning rubidium is more reactive than its predecessor, potassium, but less so than cesium. A hallmark of alkali metal reactions is the tendency to result in an alkaline solution when reacting with water, as in the case with rubidium:
\[2\mathrm{Rb(s)} + 2\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2\mathrm{RbOH}(aq) + \mathrm{H}_{2}(g)\].
It's also worth noting that when alkali metals react with halogens, they form ionic compounds, known as salts, which are highly stable due to the complete transfer of electrons:
\[2\mathrm{Rb(s)} + \mathrm{Cl}_{2}(g) \longrightarrow 2\mathrm{RbCl}(s)\].
These reactions are not only fundamental in chemistry but also have practical applications in creating a variety of products, from biofuels to pharmaceuticals.

In a synthesis chemical reaction, multiple reactants combine to form a single, more complex product. This is one of the most basic types of chemical reactions useful in understanding how compounds are formed. An essential feature of a synthesis reaction is building complexity, usually from elements or simpler compounds. For example, when rubidium reacts with chlorine gas:
\[2\mathrm{Rb(s)} + \mathrm{Cl}_{2}(g) \longrightarrow 2\mathrm{RbCl}(s)\],
the metallic rubidium and gaseous chlorine combine to yield solid rubidium chloride. Another key point about synthesis reactions is that they often release energy in the form of light or heat, thereby being exothermic. Educators need to emphasize the importance of balancing these reactions to uphold the law of conservation of mass, which is pivotal for students to learn early in their chemistry education.