![]() ![]() Later, scientists realized that the metal atom gains electrons in this process. Antoine Lavoisier demonstrated that this loss of weight was due to the loss of oxygen as a gas. In other words, ore was "reduced" to metal. The word reduction originally referred to the loss in weight upon heating a metallic ore such as a metal oxide to extract the metal. Electron donors can also form charge transfer complexes with electron acceptors. And, because it donates electrons, the reducing agent is also called an electron donor. The reductant (reducing agent) transfers electrons to another substance and is thus itself oxidized. Substances that have the ability to reduce other substances (cause them to gain electrons) are said to be reductive or reducing and are known as reducing agents, reductants, or reducers. Oxidizers are oxidants, but the term is mainly reserved for sources of oxygen, particularly in the context of explosions. O 2, F 2, Cl 2, Br 2, I 2) that can gain extra electrons by oxidizing another substance. Oxidants are usually chemical substances with elements in high oxidation states (e.g., HĤ), or else highly electronegative elements (e.g. And, because it "accepts" electrons, the oxidizing agent is also called an electron acceptor. The oxidant (oxidizing agent) removes electrons from another substance, and is thus itself reduced. Substances that have the ability to oxidize other substances (cause them to lose electrons) are said to be oxidative or oxidizing, and are known as oxidizing agents, oxidants, or oxidizers. Ultimately, the meaning was generalized to include all processes involving the loss of electrons. Later, the term was expanded to encompass oxygen-like substances that accomplished parallel chemical reactions. Oxidation originally implied a reaction with oxygen to form an oxide. The oxidation alone and the reduction alone are each called a half-reaction because two half-reactions always occur together to form a whole reaction. A redox couple is a reducing species and its corresponding oxidizing form, e.g., Fe 2+ The pair of an oxidizing and reducing agent that is involved in a particular reaction is called a redox pair. Thus, in the reaction, the reductant or reducing agent loses electrons and is oxidized, and the oxidant or oxidizing agent gains electrons and is reduced. In redox processes, the reductant transfers electrons to the oxidant. The processes of oxidation and reduction occur simultaneously and cannot occur independently. "Redox" is a combination of the words "reduction" and "oxidation". In hydrogenation, C=C (and other) bonds are reduced by transfer of hydrogen atoms. Although oxidation reactions are commonly associated with the formation of oxides, other chemical species can serve the same function. For example, in the rusting of iron, the oxidation state of iron atoms increases as the iron converts to an oxide, and simultaneously the oxidation state of oxygen decreases as it accepts electrons released by the iron. Atom transfer – An atom transfers from one substrate to another.This type of redox reaction is often discussed in terms of redox couples and electrode potentials. Electron-transfer – Only one (usually) electron flows from the reducing agent to the oxidant.There are two classes of redox reactions: Oxidation is the loss of electrons or an increase in the oxidation state, while reduction is the gain of electrons or a decrease in the oxidation state. Redox ( reduction–oxidation, / ˈ r ɛ d ɒ k s/ RED-oks, / ˈ r iː d ɒ k s/ REE-doks ) is a type of chemical reaction in which the oxidation states of substrate change. Example of a reduction–oxidation reaction between sodium and chlorine, with the OIL RIG mnemonic ![]()
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