In redox reactions, the substance that gains electrons is called an oxidizing agent, and the substance that loses electrons is called a reducing agent. In a narrower sense, an oxidizing agent can also refer to a substance that can give oxygen to another substance; similarly, a fluorinating agent is a substance that can give fluorine to a substance, as are chlorinating agents, brominating agents, etc.
An oxidizing agent is a substance that gains electrons and undergoes reduction in a redox reaction. Its oxidizing power is determined by the electron-gaining tendency of the higher-valence element and can be measured by the standard hydrogen electrode potential. Oxygen-containing oxidizing agents are more active under acidic conditions because the X-O bond is unstable, while substances with higher molecular symmetry (such as perchlorate ions) have weaker oxidizing power. Based on their electron-gaining ability, they can be divided into three categories: strong, medium, and weak, with oxygen (standard potential 1.229V) and iron ions (0.771V) as the dividing line. Based on chemical composition, they are divided into inorganic and organic oxidizing agents, and based on the reaction medium, they are divided into acidic (such as sodium dichromate), basic (such as sodium hypochlorite), and neutral (such as iodine). It is widely used in metallurgical purification and battery manufacturing. When storing, it must be kept away from organic matter and acids to avoid decomposition caused by heat or moisture.
