Oxidizing agents cause the oxidation of another substance by being reduced in a chemical reaction. They are used in various industries and products. Oxidation and reduction chemistry involve the movement of electrons between chemical species. The strength of an oxidizing agent can be estimated by its oxidation state and standard electrode potential. Oxidizers are used in industries such as chemical manufacturing, cleaning solutions, explosives, and special effects. However, they can be hazardous and require caution when handling.
In oxidation and reduction chemistry, an oxidizing agent is a substance that is reduced in a chemical reaction, thereby causing the oxidation of another substance. Common oxidizing agents include oxygen (O2), which provides the origin of the term “oxidation”, hydrogen peroxide (H2O2), ozone (O3), and halogen gases. Oxidizing agents, also known as oxidizers, are used in a wide variety of industries and products ranging from chemical manufacturing and explosives to cleaning solutions, antiseptics and special effects devices.
Oxidation and reduction chemistry, also known as redox chemistry, is the study of chemical reactions by which electrons are moved from one chemical species to another. In this reaction, the reducing agent loses electrons and becomes oxidized, while the oxidizing agent gains more electrons and becomes reduced. The OIL RIG mnemonic, which stands for “Oxidation Is Losing (electrons), Reduction Is Gaining (electrons),” is often used by chemistry students to distinguish between the two. Traditionally, the oxidizing agent was thought to be a chemical that supplied oxygen or extracted hydrogen, but the safer definition is that an oxidizing agent gains electrons and is reduced in the reaction.
The strength of an oxidizing agent can be estimated from several factors. Typically, compounds with high oxidation states, such as nitrates (NO3-), permanganates (MNO4-), and chromates (CrO42-) are good oxidizers. As a general rule, good reducing agents are bad oxidizing agents and good oxidizing agents are bad reducing agents. Another way to estimate the relative strength of an oxidizer is to determine its standard electrode potential, measured in volts. Higher potentials in the cathodic half-reaction typically correspond to higher oxidizing forces.
Oxidizers are widely used in a number of industries, from chemical manufacturing to those producing cleaning solutions and solvents, fireworks and explosives, and special effects. Sodium hypochlorite (NaClO) solutions, more commonly known as bleach, are commonly used in household cleaning applications due to their ability to remove stains. Fireworks, a common sight at nighttime outdoor celebrations, use strong oxidants to create terrifying explosions. In the special effects industry, oxidizers can be used to give new furniture a worn, aged look.
When working with oxidizing agents, it is extremely important for a chemist or student to be aware of the potential for explosion and fire hazards. Extremely strong oxidizers such as fluorine gas can react violently with reducing agents and corrode laboratory equipment. Oxygen-enriched atmospheres or pure oxygen streams can also present laboratory fire hazards. Most materials that pose a threat as strong oxidizers are accompanied by a warning or are designated as such in the United States by the letters OX in the National Fire Protection Association (NFPA) diamond special hazards section of the label.
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