Why are oxidation and reduction said to be complementary processes?

Chemical reactions are the processes where substances interact to form new substances. They involve breaking old bonds and forming new ones. Chemical reactions can be represented by balanced equations, showcasing the conversion of reactants to products. In the context of oxidation and reduction, these reactions always involve electron transfer. Think of chemical reactions like making a cake: ingredients (reactants) combine and interact to form a cake (products). Sometimes, you need to follow specific steps to get the desired result.

Electron transfer is the movement of electrons from one atom or molecule to another. This movement is crucial in oxidation and reduction processes. When a substance loses electrons, it undergoes oxidation. When another substance gains those electrons, it undergoes reduction. Imagine electrons as little balls being passed around. If one friend (atom) hands over a ball (electron) to another friend, the first friend is oxidized, and the second friend is reduced.

• Oxidation: Losing electrons
• Reduction: Gaining electrons

Without electron transfer, oxidation and reduction reactions wouldn't occur.

The oxidation state, also known as the oxidation number, is a value that helps us keep track of electrons in atoms during chemical reactions. It's especially useful for redox reactions (reactions involving both oxidation and reduction). When an atom's oxidation state increases, it means the atom has lost electrons (oxidation). When an atom's oxidation state decreases, it means the atom has gained electrons (reduction).
Think of oxidation states as scores in a game. If your score goes up, you've lost some tokens (electrons). If your score goes down, you've gained some tokens (electrons). Keeping track of these scores helps us understand and predict the behavior of substances in a chemical reaction.