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If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. All content published on the ReAgent.co.uk blog is for information only. The blog, its authors, and affiliates cannot be held responsible for any accident, injury or damage caused in part or directly from using the information provided. Additionally, we do not recommend using any chemical without reading the Material Safety Data Sheet (MSDS), which can be obtained from the manufacturer. You should also follow any safety advice and precautions listed on the product label. If you have health and safety related questions, visit HSE.gov.uk.Oxidation is the reaction caused by contact between substances and oxygen molecules. Such substances may be metals or non-metals, such as living tissues. More technically, oxidation can be defined as the loss of one electron during the phase where two or more elements interact. In this, the elements do not necessarily include oxygen. In short, it can be described as an atom’s enhanced oxidation state via a chemical reaction. It's exact opposite is called reduction, which exhibits a decrease in its oxidation state. Both reactions entail formal electron transfers. Net loss involves oxidation while net gain is the state of reduction. Advertisement Corrosionpedia Explains OxidationOftentimes, oxidation is intertwined with the term "rusting." However, not all substances that come in contact with oxygen crumble into rust. For instance, iron that is exposed to oxygen will undergo a deliberate burning process resulting in rusting. When this reaction occurs with copper, the outcome is called copper oxide, a greenish type of coating. In such a case, the metal is not waned by the oxidation process, but the material surface will form patina years after exposure to water and air. With such, corrosion can be closely associated with oxidation since the process entails bond formation between oxygen and steel. However, oxygen is not the only element that is responsible for the process of oxidation. In dry settings, most materials such as steel do not undergo rusting. The oxidation cause in such cases can be related to the existence of water. To prevent corrosion caused by oxidation, materials can be guarded through different factory coatings. These may include:
Moreover, field-applied coatings can also be utilized like those that are bitumen based, multiple- or single-layer butyl tapes, petrolatum and others. The type of coating that should be chosen depends on factors like:
By understanding the oxidation process that can be attributed to corrosion, proper coating applications can be facilitated. \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\)
This page discusses the various definitions of oxidation and reduction (redox) in terms of the transfer of oxygen, hydrogen, and electrons. It also explains the terms oxidizing agent and reducing agent. Oxidation and reduction in terms of oxygen transferThe terms oxidation and reduction can be defined in terms of the adding or removing oxygen to a compound. while this is not the most robust definition, as discussed below, it is the easiest to remember. Oxidation and Reduction with respect to Oxygen Transfer
For example, in the extraction of iron from its ore:  Because both reduction and oxidation are occurring simultaneously, this is known as a redox reaction. An oxidizing agent is substance which oxidizes something else. In the above example, the iron(III) oxide is the oxidizing agent. A reducing agent reduces something else. In the equation, the carbon monoxide is the reducing agent.
Oxidation and reduction in terms of hydrogen transferThese are old definitions which are no longer used, except occasionally in organic chemistry. Oxidation and Reduction with respect to Hydrogen Transfer
Notice that these are exactly the opposite of the oxygen definitions (#1). For example, ethanol can be oxidized to ethanal: An oxidizing agent is required to remove the hydrogen from the ethanol. A commonly used oxidizing agent is potassium dichromate(VI) solution acidified with dilute sulfuric acid. Ethanal can also be reduced back to ethanol by adding hydrogen. A possible reducing agent is sodium tetrahydridoborate, NaBH4. Again the equation is too complicated to consider at this point. More precise definitionsof oxidizing and reducing agents are
Oxidation and reduction in terms of electron transferOxidation and Reduction with respect to Electron Transfer
Remembering these definitions is essential, and easily done using this convenient acronym: Example 1 The equation below shows an obvious example of oxygen transfer in a simple redox reaction: \[ \ce{CuO + Mg \rightarrow Cu + MgO} \nonumber\] Copper(II) oxide and magnesium oxide are both ionic compounds. If the above is written as an ionic equation, it becomes apparent that the oxide ions are spectator ions. Omitting them gives: In the above reaction, magnesium reduces the copper(II) ion by transferring electrons to the ion and neutralizing its charge. Therefore, magnesium is a reducing agent. Another way of putting this is that the copper(II) ion is removing electrons from the magnesium to create a magnesium ion. The copper(II) ion is acting as an oxidizing agent. SummaryConfusion can result from trying to learn both the definitions of oxidation and reduction in terms of electron transfer and the definitions of oxidizing and reducing agents in the same terms. The following thought pattern can be helpful:
Here is another mental exercise:
This page titled Definitions of Oxidation and Reduction is shared under a not declared license and was authored, remixed, and/or curated by Jim Clark. What is oxidation process explain with example?The term oxidation was originally used to describe reactions in which an element combines with oxygen. Example: The reaction between magnesium metal and oxygen to form magnesium oxide involves the oxidation of magnesium.
What is the oxidation process called?The chemical reactions which involve the transfer of electrons from one chemical substance to another. These electron-transfer reactions are termed as oxidation-reduction reactions or redox reactions.
What are the 2 processes of oxidation?Oxidation as a gain of oxygen – An oxidizing agent gives oxygen atoms to another substance in a compound. Oxidation as a loss of hydrogen – An oxidizing agent removes hydrogen atoms from another substance in a compound.
Where the process of oxidation occurs?Oxidation occurs when an atom, molecule, or ion loses one or more electrons in a chemical reaction. When oxidation occurs, the oxidation state of the chemical species increases. Oxidation doesn't necessarily involve oxygen! Originally, the term was used when oxygen caused electron loss in a reaction.
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