Hydrogen, which has a solitary electron in its orbit, loses it, and chlorine, which has 17 electrons in a stable state, gains one electron. In this reaction, two sub-reactions are occurring: The oxidation of hydrogen, and the reduction of chlorine. An easily understood example of redox reactions is the formation of acids. Thus, these two reactions always occur in conjunction with each other. Because two entities must partake in a redox reaction, one loses atoms, which the other gains. Oxidation is the process of losing an electron, whereas reduction, though it may seem incorrectly named, is the process of gaining an electron. Its name is a portmanteau of the two processes or sub-reactions that inevitably occur in it― reduction and oxidation.
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A redox reaction, one of the most fundamental and commonly seen principles of chemistry, is a reaction where electrons are transferred between two atoms/molecules. The oxidation number of an atom simply shows the number of electrons it can account for in a redox reaction, or the degree to which it has undergone oxidation. But first, let’s understand what oxidation numbers are in the first place. Here is a helpful guide on the steps to determine the oxidation number of elements. Though it is so fundamental, some may not understand the confusing rules of determining oxidation numbers.
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It is one of the most basic principles of chemistry, and plays a determinant role in the nature of many types of reactions. Oxidation state, denoted by the oxidation number, is a very important concept in chemistry. Did You Know?Ĭarbon has 9 possible oxidation states―from -4 to +4. It is crucial in understanding the nature of various reactions. Oxidation number/state is an important but very often misunderstood concept.