Profile
Settings
Refer your friends
Sign out
When the oxidation state of a molecule, atom, or ion increases, this is referred to as oxidation. Alternatively, reduction occurs when an increase in the number of electrons is seen or when the oxygenation state of an atom, molecule, or ion is found to be lower than normal.
Oxidation in the context of oxygen is defined historically.
When oxygen was added to a chemical, this was referred to as oxidation in an older sense. This was due to the fact that oxygen gas (O2) was the very first oxidising agent ever discovered. The addition of oxygen to a substance normally satisfies the criteria of electron loss and an increase in the oxidation state; however, the concept of oxidation has been broadened to cover a wide variety of chemical processes.
When iron reacts with oxygen to generate iron oxide, sometimes known as rust, this is a classic illustration of the classical concept of oxidation. It is believed that the iron has oxidised and turned into rust.
Fe2O3 is formed when two iron atoms combine with oxygen.
Rust is formed when the iron metal is oxidised, resulting in the formation of iron oxide.
Oxidation reactions, such as electrochemical reactions, are excellent examples. When a copper wire is immersed in a solution containing silver ions, electrons are transferred from the copper metal to the silver ions, resulting in the formation of silver ions. Occurrence of oxidation in copper metal. Whiskers of silver metal are formed on the copper wire, and copper ions are discharged into the solution as a result.
Cu(s) + 2 Ag+(aq) ←→ Ag(s) + Cu2+(aq)
One such example of oxidation, in which an element joins with oxygen, is the reaction between magnesium metal and oxygen, which results in the formation of magnesium oxide.
Redox reactions
Oxidation and reduction are two different processes, known as redox reaction. The discovery of the electron, as well as the ability to describe chemical reactions, led scientists to recognise that oxidation and reduction occur in tandem, with one species losing electrons (oxidised) and another receiving electrons (reduced) (reduced). A redox reaction is a type of chemical process in which both oxidation and reduction take place. The term “redox reaction” is an abbreviation for “reduction-oxidation.”
The oxidation of a metal by oxygen gas might potentially be explained by the metal atom losing electrons to generate the cation (which is being oxidised) while the oxygen molecule gains electrons to form oxygen anions (which are being reduced).
It is made up of the following two half-reactions:
Mg2+ + 2 e- → 2Mg
2 O2- → O2 + 4 e-
The Definition of Oxidation Involving Hydrogen Throughout History
According to the contemporary definition of the term, oxidation in which oxygen is involved is still considered to be oxidation. However, there is another old definition using hydrogen that may be found in organic chemistry textbooks and is worth mentioning. This term is diametrically opposed to the definition of oxygen, and as a result, it may generate confusion. Nonetheless, it is beneficial to be informed. According to this definition, oxidation is defined as the loss of hydrogen, whereas reduction is defined as the acquisition of hydrogen.
When ethanol is converted to ethanal, for example, the following occurs according to this definition:
CH3CH2OH → CH3CHO + H2
Because it has lost hydrogen, ethanol is thought to be oxidised. In the opposite direction of the equation, ethanal can be decreased by adding hydrogen to it, resulting in the formation of ethanol.
Conclusion
Therefore it can be concluded, Making Use of the OIL RIG to Recall Oxidation and Reduction
So keep in mind that the contemporary definitions of oxidation and reduction are concerned with electrons and protons (not oxygen or hydrogen). The acronym OIL RIG can be used to keep track of which species is oxidised and which species is reduced. OIL RIG is an abbreviation for Oxidation Is Loss, Reduction Is Gain, which stands for Oxidation Is Loss, Reduction Is Gain.
