## Redox Reactions Chemical reactions that achieve a state of valence equilibrium are known as redox reactions, which include two key processes: reduction and oxidation. In these reactions, "reduction" refers to the gain of electrons by a molecule, atom, or ion, while "oxidation" pertains to the loss of electrons. These processes occur simultaneously, with the substance that gains electrons being reduced and the one that loses electrons being oxidized. Together, they facilitate the transfer of electrons between substances, enabling the complex changes essential for numerous biological and chemical processes. ### Reducing Reaction A simple way you can remember reducing reactions is through the idea that reducing looks like. a minus sign, so at the end of the reaction, the element is an anion, thereby it has an abundance of electrons. ### Oxidative Reaction ### Ionic vs Covalent Redox Reactions ### Ionic Reactions In ionic redox reactions, the redox process results in an anion and a cation. Two atoms or molecules that were originalyl electrivally neutral are now not, because one has an abundance of electrons (is reduced) and the other has an absence of electrons (is oxidized).  ### Covalent Reactions In covalent redox reactions, the ![[Chemistry - Polar Bond in Hydrogen Chloride Molecule.mp4]] These two approaches to equilibrium highlight the essential principles of atomic structure and chemistry, illustrating the inherent order within the microscopic world.