Jonah Patel
Oxidation-reduction reactions, also known as redox reactions, are chemical reactions that involve the transfer of electrons between two species. The original meaning of the term oxidation described reactions in which an element combines with oxygen. However, after the discovery of electrons, oxidation was redefined as the loss of electrons. In redox reactions, one reactant loses electrons (oxidation) while the other gains them (reduction), and these reactants are known as the oxidizing and reducing agents, respectively. Redox reactions are essential to basic life functions such as photosynthesis, respiration, and combustion.
| Characteristics | Values |
|---|---|
| Type of chemical reaction | Oxidation-reduction (redox) reaction |
| Definition | A chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron |
| Oxidation state | The oxidation state of an atom is the charge that atom would carry if the compound were purely ionic |
| Oxidation | The loss of electrons or hydrogen |
| Reduction | The gain of electrons or hydrogen |
| Oxidizing agent | The ion or molecule that accepts electrons and oxidizes another substance |
| Reducing agent | The ion or molecule that donates electrons and reduces another substance |
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What You'll Learn
Oxidation is the loss of electrons
Oxidation-reduction reactions (also known as redox reactions) are chemical reactions in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. These reactions are common and vital to some of the basic functions of life, including photosynthesis, respiration, combustion, and corrosion or rusting. The oxidation state (OS) of an element corresponds to the number of electrons that an atom loses, gains, or appears to use when joining with other atoms in compounds.
In oxidation-reduction reactions, there is an oxidizing agent and a reducing agent. The ion or molecule that accepts electrons is the oxidizing agent, and by accepting electrons, it oxidizes other species. The ion or molecule that donates electrons is the reducing agent, and by giving electrons, it reduces the other species. For example, when magnesium reacts with oxygen, the magnesium atoms donate electrons to O2 molecules, thereby reducing the oxygen. The O2 molecules gain electrons from magnesium atoms, thereby oxidizing the magnesium.
There are various mnemonic devices to help remember the relationship between oxidation and reduction, including OIL RIG, which stands for "oxidation is loss" and "reduction is gain." Another is LEO the lion says GER, which stands for "loss of electrons is oxidation, gain of electrons is reduction."
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Reduction is the gain of electrons
Oxidation-reduction reactions, or redox reactions, are chemical reactions in which electrons are transferred between two species. These reactions are fundamental to many basic life functions, including photosynthesis, respiration, combustion, and corrosion. In a redox reaction, one substance loses electrons (oxidation) while another gains electrons (reduction), and these two processes always occur together.
The gain of electrons by the oxidizing agent leads to a decrease in its oxidation state. The oxidation state, or oxidation number, of an element corresponds to the number of electrons it loses, gains, or appears to use when joining with other atoms in compounds. For instance, in the rusting of iron, the oxidation state of iron atoms increases as they lose electrons, while the oxidation state of oxygen decreases as it gains electrons.
Reducing agents, or reductants, are substances that cause other substances to gain electrons. They transfer electrons to another substance, thereby reducing it. Reducing agents are also called electron donors due to their ability to donate electrons. Electropositive elemental metals such as lithium, sodium, magnesium, iron, zinc, and aluminium are good examples of reducing agents as they readily donate electrons.
To summarise, reduction is the gain of electrons in a redox reaction. The oxidizing agent is responsible for this gain of electrons, while the reducing agent loses electrons and is itself oxidised. The oxidation and reduction processes occur simultaneously and are integral to many chemical reactions.
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Oxidation and reduction always occur together
Oxidation and reduction reactions, also known as redox reactions, always occur together. These reactions are common and vital to some of the basic functions of life, including photosynthesis, respiration, combustion, and corrosion or rusting.
Redox reactions involve the transfer of electrons between two species. One species is oxidized (loses electrons), while another species is reduced (gains electrons). For example, in the reaction between hydrogen peroxide (H2O2) and potassium permanganate (KMnO4), hydrogen peroxide is oxidized, and potassium permanganate is reduced.
The two species that exchange electrons in a redox reaction are given special names. The ion or molecule that accepts electrons is called the oxidizing agent, while the ion or molecule that donates electrons is called the reducing agent. For instance, when magnesium reacts with oxygen, the magnesium atoms donate electrons to O2 molecules, thereby reducing the oxygen. Here, magnesium acts as the reducing agent, and oxygen is the oxidizing agent.
It is important to note that oxidation and reduction can be defined in terms of the gain or loss of hydrogen atoms as well. If a molecule adds hydrogen atoms, it is being reduced, and if it loses hydrogen atoms, it is being oxidized.
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Oxidation involves the addition of oxygen
The term oxidation was originally used to describe reactions in which an element combines with oxygen. For example, the reaction between magnesium metal and oxygen to form magnesium oxide involves the oxidation of magnesium. However, the modern definition of oxidation is more general and involves the loss of electrons during a reaction by a molecule, atom, or ion. This loss of electrons often coincides with the addition of oxygen to a compound, as oxygen is electronegative and attracts electrons from other atoms.
Oxidation is the addition of oxygen to a compound, which often results in the loss of electrons from that compound. This definition is useful for remembering the process of oxidation, although it is not the most robust definition. In the extraction of iron from its ore, both reduction and oxidation occur simultaneously, and this is known as a redox reaction. An oxidizing agent is a substance that adds oxygen to another substance, causing it to oxidize. For example, when magnesium reacts with oxygen, the magnesium atoms donate electrons to O2 molecules, thereby reducing the oxygen. The O2 molecules gain electrons from magnesium atoms, thereby oxidizing the magnesium.
Oxidation can also be defined in terms of the gain or loss of an electron. The reaction in which a molecule, atom, or ion loses an electron is called an oxidation reaction. The oxidation state of a molecule, atom, or ion is its oxidation number, and this number increases in an oxidation reaction. An atom is oxidized if its oxidation number increases, and reduced if its oxidation number decreases. For example, when copper is heated over a flame, the surface slowly turns black as the copper metal reduces oxygen in the atmosphere to form copper(II) oxide.
Oxidation can also be defined in terms of changing the oxidation state. The reaction in which there is an increase in the oxidation state is called an oxidation reaction. The oxidation state of an individual atom is 0, and the total oxidation state of all atoms in a neutral species is 0. In an ion, the total oxidation state is equal to the ion charge. For example, in the reaction between hydrogen and fluorine gas to form hydrofluoric acid, oxidation occurs as there is a loss of electrons.
While oxidation was originally defined as the addition of oxygen to a compound, the modern definition is more general and involves the loss of electrons. This is because not all oxidation reactions involve the addition of oxygen, and the definition has been expanded to include other types of chemical reactions. However, oxidation reactions that do involve the addition of oxygen often result in the loss of electrons, as oxygen is electronegative and attracts electrons from other atoms.
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Reduction involves the removal of oxygen
Oxidation-reduction (redox) reactions are chemical reactions that involve the transfer of electrons between two species. In redox reactions, one reactant is oxidised (loses electrons) and the other is reduced (gains electrons). The term "oxidation" was originally used to describe reactions in which an element combines with oxygen. For example, when magnesium reacts with oxygen, the magnesium atoms donate electrons to oxygen molecules, reducing the oxygen. Therefore, the removal of oxygen is a reduction reaction.
The word "reduction" comes from the Latin stem meaning "to lead back". Reduction involves the removal of oxygen from another substance. For example, the reaction between magnesium oxide and carbon at 2000°C results in the reduction of magnesium oxide to magnesium metal. In this reaction, the carbon monoxide is the reducing agent.
Reduction can also be defined as the gain of hydrogen. For example, ethalan can be reduced back to ethanol by adding hydrogen. Sodium tetrahydridoborate (NaBH4) is a possible reducing agent in this reaction.
In the context of electrochemical reactions, oxidation and reduction processes occur simultaneously but are separated in space. An example of this is cellular respiration, which involves the oxidation of glucose (C6H12O6) to CO2 and the reduction of oxygen to water.
It is important to note that the definitions of oxidation and reduction based solely on the transfer of oxygen are old definitions that are no longer commonly used, except occasionally in organic chemistry. More precise definitions of oxidation and reduction focus on the transfer of electrons and changes in oxidation states.
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Frequently asked questions
Oxidation reactions are chemical reactions where an atom or ion loses one or more electrons. The molecule that gains electrons is called the oxidizing agent.
Reduction reactions are chemical reactions where an atom or ion gains one or more electrons. The molecule that loses electrons is called the reducing agent.
Oxidation and reduction reactions are two sides of the same coin, always occurring together. This is because electrons are neither created nor destroyed in a chemical reaction, so if one reactant loses an electron (oxidation), another must gain it (reduction).
To identify an oxidation reaction, you need to determine if there is a change in the oxidation state of the atoms, ions, or molecules involved. If there is a loss of electrons, it is an oxidation reaction.
