What are oxidising agents

In order to oxidize a substance, there must be an oxidizing agent present. What is an oxidizing agent? An oxidizing agent is defined as a compound that can be easily reduced, thereby gaining electrons. In the process of gaining electrons, oxidization of the other substance occurs. An oxidizing agent can also be referred to as an oxidizer, meaning compounds that can oxidize. Although this concept can become slightly confusing, because the oxidizing agent is ultimately the substance that gets reduced via electron gain, it may help to remember that an oxidizer is the agent that brings about oxidation. Since oxidation must result in an opposite reduction happening, the reduction happens on the oxidizing agent. The terms oxidation and reduction are referring to an increase or decrease in the oxidation state. The following key points are important for understanding oxidation and reduction: What is an Oxidizing Agent? Have you ever seen a rusted nail or spoiled food? These are the end results of processes that involve oxidizing agents. Oxidizing agents are substances that gain electrons in a chemical reaction. Because of this action, oxidizing agents are also known as electron acceptors. Let's put this in more visual terms. We just learned that oxidizing agents accept electrons. Let's recall that electrons are particles that have a negative charge. When oxidizing agents gain a negative charge, it can be said that they are reduced, as shown in this diagram: The reason why a substa...

Oxidizing Agent What is an Oxidizing Agent? An oxidizing agent (often referred to as an oxidizer or an oxidant) is a chemical species that tends to oxidize other substances, i.e. cause an increase in the oxidation state of the substance by making it lose electrons. Common examples of oxidizing agents include halogens (such as chlorine and fluorine), oxygen, and hydrogen peroxide (H 2O 2). Table of Contents • • • • Definition Oxidizing agents can be defined in two different ways: As an electron acceptor– They are chemical substances whose atoms remove at least one electron from another atom in a chemical reaction. As per this definition, oxidizing agents are the reactants that undergo reduction in Here, substance ‘A’ undergoes oxidation, resulting in an increase in its oxidation number. On the other hand, the oxidation state of substance ‘B’ becomes smaller (since it gains electrons by undergoing reduction). Click here to learn As an atom-transferring substance– An oxidizing agent is a substance that transfers at least one electronegative atom to a chemical species in a chemical reaction. The transferred atom is typically an oxygen atom. Several combustion reactions and organic redox reactions involve the transfer of an electronegative atom between two reactants. In the example illustrated above, the Fe 2O 3 molecule acts as an oxidizer by transferring an electronegative oxygen atom to the carbon monoxide molecule. What Factors Affect the Oxidizing Power of an Oxidi...

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\( \newcommand\) • • • • • • • Oxidizing and reducing agents are key terms used in describing the reactants in redox reactions that transfer electrons between reactants to form products. This page discusses what defines an oxidizing or reducing agent, how to determine an oxidizing and reducing agent in a chemical reaction, and the importance of this concept in real world applications. Oxidizing and Reducing Agents An oxidizing agent, or oxidant, gains electrons and is reduced in a chemical reaction. Also known as the electron acceptor, the oxidizing agent is normally in one of its higher possible oxidation states because it will gain electrons and be reduced. Examples of oxidizing agents include halogens, potassium nitrate, and nitric acid. A reducing agent, or reductant, loses electrons and is oxidized in a chemical reaction. A reducing agent is typically in one of its lower possible oxidation states, and is known as the electron donor. A reducing agent is oxidized, because it loses electrons in the redox reaction. Examples of reducing agents include the earth metals, formic acid, and sulfite compounds. Figure \(\PageIndex\) Halogens (they favor gaining an electron to obtain a noble gas configuration) Alkali metals (they favor losing an electron to obtain a noble gas configuration) Exercise\(\PageIndex\) is the oxidizing agent. Note that while a specific atom typically has an odization state changes, the agents are the actual species, not the atoms. Applications Oxidizing...

Oxidising agent example refers to reduced elements, which separate electrons from other elements in Redox reactions. Let us describe the examples. The Oxidising agent examples are listed below: • Halogen elements (Cl, Br, I, F) • • Hydrogen peroxide (H2O2) • Potassium permanganate (KMnO4) • Potassium dichromate (K2Cr2O7) • Nitric acid (HNO3) • Carbon dioxide (CO2) • • • Water (H2O) • • • Halogen elements (Cl, Br, I, F) Electron affinity refers to an urge of element to have electrons in the empty space of its valence shells. Electronegativity of elements refers to urge of taking electrons in itself. The tendency of halogens to attract the electrons and making halide ions is the key reason that makes them strong oxidising agent. Oxygen (O2) Oxygen is the most effective example of oxidising agent. This element is highly valuable in the regular life of people. It works as an oxidiser being reduced while making rust, supporting the human body in breathing and facilitating living beings to do aerobic respiration. It is considered as oxidiser. Hydrogen peroxide (H2O2) Hydrogen peroxide is an oxidising agent as it can be reduced readily to convert Carboxylic acid to peroxy acid. However, Hydrogen peroxide is the same kind of oxidiser as oxygen but is more powerful than Oxygen. As this compound holds one more Oxygen, it impose strong oxidation than normal Oxygen molecule. Potassium permanganate (KMnO4) KMnO4 is a reliable example of strong oxidising agent. The oxidation state of th...

Recent Examples on the Web This is because bleach contains harsh oxidizing agents that hair-color remover does not. — Marisa Petrarca, Allure, 2 Mar. 2023 Another group exposed nanotubes to sulfuric acid and potassium permanganate, a strong oxidizing agent, which strained the carbon bonds and caused the tubes to unzip lengthwise, as shown here. — Discover Magazine, 29 June 2010 Once a missile appears to be fueled, analysts assume it will be launched within three to four days because a corrosive oxidizing agent in the fuel could cause a leak if the delay exceeds that. — Alastair Gale, WSJ, 27 May 2022 In a rocket engine, chamber pressure refers to the amount of fuel and oxidizing agent that can be mixed and ignited, which then generates thrust to lift the rocket. — Christiaan Hetzner, Fortune, 14 Feb. 2022 This by itself was alarming, but not unprecedented: Liquid propellants, long preferred in many Russian missiles, are volatile and have exploded when prematurely brought into contact with oxidizing agents. — Ankit Panda, The New Republic, 21 Aug. 2019 These examples are programmatically compiled from various online sources to illustrate current usage of the word 'oxidizing agent.' Any opinions expressed in the examples do not represent those of Merriam-Webster or its editors.

The best reducing agents are located at the bottom left of the periodic table (low electronegativity) and the best oxidizing agents are located at the top right of the periodic table (high electronegativity), excluding noble gases. Is electronegativity the factor that determines the strength of reducing agents and oxidizing agents? $\begingroup$ The strength of reducers and oxidizers depends upon the thermodynamic favorability of their reactions. The strongest elemental reducing agent is lithium, which is not the least electronegative element. When Li acts as a reducing agent, metallic bonds are broken and one electron is removed from each Li atom. These processes are endothermic. The Li is solvated (exothermic). For an oxidizer like chlorine, the Cl-Cl bond is broken (endothermic) then the Cl gains an electron (exothermic). The chloride is solvated (exothermic). All this adds up to how favorable the reduction is. $\endgroup$ Because compounds can be oxidizing agents like potassium permangenate (KMnO 4) and reducing agents LiH 4, what makes a compound an oxidizing or reducing agent is oxidation & reduction tables. As oxidation is the giving off of electrons and reduction is the acceptance of electrons, like plus vs minus relationship, if you have an oxidation table you can turn it into a reduction table by putting the flipping the table, changing the signs and reversing the equations. Anyway, reduction tables are more standard, where the strongest oxidizing agents have the...

\( \newcommand\) • • • • 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 with respect to Oxygen Transfer • Oxidation is the gain of oxygen. • Reduction is the loss of oxygen. 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. • Oxidizing agents give oxygen to another substance. • Reducing agents remove oxygen from another substance. Oxidation and Reduction with respect to Hydrogen Transfer • Oxidation is the loss of hydrogen. • Reduction is the gain of hydrogen. 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, NaBH 4. Again the equation is too complicated to consider at this point. More precise definiti...