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What are redox reactions?

What are redox reactions?

A redox reaction consists of two parts, the reduced half, and the oxidized half, which always go together. The reduced half gains electrons and the oxidation state decreases, while the oxidized half loses electrons, and the oxidation state increases. The number of electrons stays the same in a redox reaction. What is released in the oxidation half-reaction is absorbed by another particle in the reduction half-reaction. The two types of exchanging electrons in redox reactions are given special names. An ion or molecule that accepts electrons is called an oxidizer, and when it accepts electrons, it oxidizes other particles. By giving electrons it reduces the other species the ion or molecule that donates electrons is called the reducing agent. Hence, the reducing agent is what is oxidized and oxidizing agent what is reduced. The oxidizing and reducing agents are formed from same element or compound. the thermite reaction is considered as a good example of a redox reaction wherein iron atoms in ferric oxide lose O atoms to Al.

Oxidizing and reducing agents: In redox processes, in the reaction, the reductant or reducing agent loses electrons and is oxidized, and the oxidant or oxidizing agent gains electrons and is reduced thus, the reductant transfers electrons to the oxidant. The pair called a redox pair is formed of an oxidizing and reducing agent that is involved in a particular reaction.

Oxidants The international pictogram for oxidizing chemicals: Oxidizing agent Substances which have the ability to oxidize other substances (causing them to lose electrons) are called oxidants and are called oxidizing agents and is therefore itself reduced. Andit is called electron acceptor because it “accepts” electrons, the oxidizing agent is also called an. Oxygen is the oxidant par oxidizing.

Redox reaction in industry: a technique in which by making a metal surface the cathode of an electrochemical cell is used to control corrosion is called Cathodic protection. A simple method of protection connects the protected metal to a more easily corroded “sacrificial anode” that serves as the anode. The sacrificial metal corrodes instead of the metal being protected. Generally, cathodic protection is applied to galvanized steel, and a zinc protective coating on the steel part protects against corrosion. Oxidation is used in a variety of industries, such as manufacturing detergents and oxidizing ammonia to produce nitric acid. The redox reaction is at the heart of electrochemical cells that can generate electrical energy or support electrosynthesis. Metal ores often contain metals in oxidation states such as oxides or sulfides, and pure metals are recovered through high-temperature smelting in the presence of reducing agents. The electroplating process uses a redox reaction to coat an object with a thin layer of material, such as chrome-plated car parts, silver spoons, electroplated and gold-plated jewelry.

Redox reactions in soil Electron transfer reactions play a central role in numerous processes and properties of soil, and the “activity” of electrons quantified as Eh (potential (voltage) of a platinum electrode relative to a standard hydrogen electrode) or pe (similar to pH). The logarithmic activity of the former is the main variable. Early theoretical studies applied to flooded soil and rice production with pH controlling and regulating chemical reactions and biological processes were instructive for later studies of thermodynamic aspects of redox potentials. Plant root growth in soil [16] Further work based on this foundation has investigated the oxidation states of heavy metals, soil formation and morphology, decomposition and formation of organic compounds, free radical chemistry, wetlands, soil remediation and redox potential. Different methodological approaches to characterize. soil condition.

Do you know the answer of the below question?

  1. Oxidation number of carbon is correctly given for

A.Compound HN=→CO.N.+2CompoundO.N.HN=→C+2


C.CompoundCCl4O.N. + 4 Compound O.N. CCl4+4


Redox cycle form free radicals that contain one more electron than the parent compound where various aromatic compounds are reduced by enzymes. Typically, the electron donor is one of a variety of flavoenzymes and coenzymes. Once formed, these anionic free radicals reduce molecular oxygen to peroxide and regenerate the unaltered parent compound. The final reaction is that the coenzyme of the flavoenzyme is oxidized, and molecular oxygen is reduced to form peroxide. This catalytic behavior has been described as a useless cycle or a redox cycle.

In geology, redox potentials are important for both mineral formation and mineral mobilization and are also important in some sedimentary environments. color forms the basis of determination of the redox state of most rocks. Rocks form under oxidizing conditions, giving them a reddish color. Then, as the repair fluid passes through the rock, it “discolors” to green and sometimes turns white. The recovered fluid may also contain uranium-containing minerals. Notable examples of redox conditions that affect geological processes include uranium deposits and moquy marbles.

Biological energy is often stored and released through redox reactions. In the process of Photosynthesis carbon dioxide reduction happens to sugars while water oxidation to molecular oxygen also occurs. The reverse reaction, respiration, oxidizes sugars to produce carbon dioxide and water.

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