What are Redox reactions theory and examples?
Redox reactions theory and examples:
Redox reactions theory and examples are briefly listed here in this topic we will completely understand this concept now first discuss about what are Redox reactions
The oxidation-reduction reaction is also called the oxidation-reduction reaction, which is a chemical reaction that transfers one or more electrons from a molecule or compound to another, and the types that lose electrons are usually oxidized and are a reducing agent, while the types that gain electrons are usually an oxidizing agent, Oxidation and reduction reactions every day include photosynthesis, respiration, combustion, and corrosion .
And oxidation and reduction are always present side by side during oxidation and reduction reactions, where when an element is oxidized, another component or other compound must be reduced, that is, we must be able to Striking a balance in T. Aalat oxidation and reduction.
 The difference between oxidation and reduction:
There is a big difference between oxidation and reduction, and this difference lies in the fact that oxidation means the loss of electrons in the chemical reaction , and is associated with the process of oxidation. The reducing factor is that the reducing agent is the substance that is oxidized during the reaction, that is, it loses electrons in the oxidation and reduction reaction.
¤Redox reactions Examples :
Examples of reducing factors are terrestrial minerals. As for formic acid and sulfite compounds, the reduction means gaining electrons in the chemical reaction, and the oxidation factor is related to the reduction process as the oxidizing factor is the material that is reduced during the chemical reaction i.e. it is gaining electrons. Helm halogens and potassium nitrate and nitric acid .
 The general theory of redox reactions:
The description of the above redox processes does not convey the mechanism by which this change occurs. The full description of the net chemical change of a process is known as the measurement of the reacting elements in the reaction, which provides the property of combining the proportions of elements and compounds, and the reactions are categorized as oxidation or reduction on the basis of Measure the reactants of both the oxygen atomOr the hydrogen atom and the electron transport, and the comprehensive definitions of oxidation and reduction became possible thanks to the theory of modern molecular structure, which states that each atom consists of a positive nucleus surrounded by negative electrons that determine the bonding properties of each element, whereby when chemical bonds are formed, the atoms donate, gain, or share electrons.
This makes it possible to assign an oxidation number to each atom, and the oxidation number determines the number of electrons that can participate in forming bonds with other atoms of specific atoms in a given molecule with known bonding capabilities and the bonding pattern within the molecule is determined, and each atom is considered in a state a A certain number helm expressed oxidation.
 Redox reactions in everyday life:
Redox reactions include very many processes and interfere in wide and different applications. Among these processes are the phenomena, interactions and vital processes that occur in daily life, the most important of which are the following:
 Photosynthesis in plants:
Since in this process that occurs in the green leaves of plants , carbon dioxide and water combine under the influence of light to form molecular oxygen and glucose as glucose is used as fuel for metabolic processes, and in the first step light energy is used to release and reduce hydrogen atoms and create oxygen gas and these atoms reduce carbon In carbon dioxide, this can be expressed almost as follows: carbon dioxide + water + light energy → carbohydrates + oxygen + water.
The cellular respiration of organisms allows the release of energy stored in the chemical bonds of glucose , that is, we obtain energy from food, and the formula is as follows: C6H12O6 + 6 O2 -> 6 CO2 + 6 H2O + 36 ATP As ATP is adenosine triphosphate, it is a simple energy saving compound as it drives various metabolic processes.
Some might think that combustion is a more physical process than a chemical process, but the combustion of hydrocarbons in fossil fuels as well as the burning of organic materials in wood represent a kind of oxidation and reduction reactions, as the carbon in the compound burns with oxygen atoms in the air and the oxygen atoms are bound to the hydrogen in The compound, therefore, is the oxidizing compound that is burned and emits carbon dioxide and water vapor as combustion products.
As when contacting water with an iron pipe, for example, some of the oxygen present in the water leads to the oxidation of iron, which results in hydrogen ions, and these ions combine with the oxygen in the surrounding air to form the water, and this process starts again when the iron is oxidized, which leads to an increase The amount of oxidized iron, that is, which carries more and more positive charge, and with reactions that occur and oxidation produces our brownish substance known as rust .
You may also like that
You may also look through