Write a balanced equation for the reaction that occurs in each of the following cases: (a) Cesium is added to water. (b) Strontium is added to water. (c) Sodium reacts with oxygen. (d) Calcium reacts with iodine.

Chemical reactions are processes where reactants transform into products through breaking and forming of chemical bonds. This transformation follows the law of conservation of mass, meaning that atoms are neither created nor destroyed during a chemical reaction.

For instance, when cesium reacts with water, cesium atoms and water molecules rearrange to form new substances: cesium hydroxide and hydrogen gas. A similar transformation occurs when strontium reacts with water, producing strontium hydroxide and hydrogen gas. These reactions not only show the change from reactants to products but also the importance of balancing the equation to reflect the mass conservation law.

The reactivity of metals plays a significant role in determining how vigorously a metal reacts with other substances. Metals like cesium and sodium are highly reactive with water and oxygen due to their position in the reactivity series, a list of metals arranged according to their ability to displace other metals in a compound.

For example, cesium displaces hydrogen from water with such vigor because it is a highly reactive metal from the alkali metals group. On the other hand, calcium's reaction with iodine is less vigorous, as calcium is less reactive than cesium or sodium. Understanding the reactivity of metals helps predict the outcome of chemical reactions and the safety precautions necessary during those reactions.

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. By following the basic principle that matter cannot be created or destroyed, stoichiometry involves calculating the amounts of reactants required or products formed in a reaction.

For instance, in the reaction of sodium with oxygen, stoichiometry dictates that four sodium atoms react with one molecule of oxygen to produce two formula units of sodium oxide. Here, stoichiometry ensures the balanced equation complies with the law of conservation of mass. Students can use stoichiometric calculations to predict the amount of each substance involved, ensuring the equation is quantitatively accurate and allowing for the proper scaling of reactions for various applications.