Redox reaction

Redox reactions involve simultaneous oxidation and reduction processes. Oxidation refers to the addition of oxygen or the removal of hydrogen, whereas reduction is characterized by the addition of hydrogen or the removal of oxygen. In the electronic context, oxidation is the loss of electrons, leading to an increase in oxidation state, while reduction involves the gain of electrons and a decrease in oxidation state. The substances facilitating these processes are called agents: the oxidizing agent is the substance that gets reduced, while the reducing agent is the one that gets oxidized.

The oxidation number (O.N.) is a formal charge assigned to an atom in a molecule, with some standard rules governing its assignment. For example, elemental forms have an O.N. of 0, fluorine is always -1, oxygen is typically -2 with exceptions, and hydrogen's O.N. depends on the nature of other elements present.

Redox reactions can take various forms, including combination, decomposition, displacement, and disproportionation reactions. Normality in redox reactions is calculated using the formula Normality = Molarity × n-factor, where the n-factor represents the total change in oxidation state. In titrations, the law of equivalence states that the equivalents of the oxidizing agent must equal those of the reducing agent, and indicators are utilized to determine endpoint.

Balancing redox reactions may involve the ion-electron method, where the reaction is split into half-reactions for easier management. The Principle of Atom Conservation (POAC) can also be applied to showcase that the moles of specific atoms remain constant through the reaction process.