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In the definition of redox reactions, the transfer of electrons takes place from one reactant to another. Such electron-transfer reactions are commonly called oxidation-reduction or redox reactions. The oxidation-reduction reaction involves changes in energy in heat, electricity, light etc. Adding oxygen and hydrogen to different substances results in oxidation and reduction reactions. The process of Oxidation and Reduction occurs one after the other in an oxidation-reduction reaction. Read the whole article to gather knowledge about redox reactions.
What is meant by Oxidation?
It is an earlier or traditional concept in the definition of redox reaction. Adding oxygen or an electronegative element or removing hydrogen or an electropositive element occurs in an oxidation method. As per an electronic concept, it is a technique in which an atom or ion loses electrons.
The example of slow Oxidation:-
Iron rusting and wood-rotting both are examples of slow Oxidation.
What is meant by Reduction?
Reduction is a very useful approach in the definition of redox reaction. It is a process that involves adding hydrogen or an electropositive element or removing oxygen or an electronegative element.
It is the opposite of the oxidation process since an atom or ion gains electrons in Reduction.
One of the huge differences between Reduction and Oxidation is that, In the definition of a redox reaction, Reduction is the gaining of electrons and Oxidation is the loss of electrons.
About standard electrode potential of hydrogen
The standard electrode potential of hydrogen is equal to zero at all temperatures. Because earlier, the potential is assumed to be zero.
An electrochemical cell, the standard electrode potential can have the temperature = 298K, pressure = 1atm, concentration = 1M. The standard electrode potential uses the symbol ‘Eocell’ to represent.
Table of standard reduction potentials
This table of standard reduction potentials is used to give the Eo for specified reduction reactions.
It follows an order that the stronger (more reactive) reductants stay at the top, and the stronger oxidants stay at the bottom :-
The Oxidation and Reduction reactions involve:
Oxidation reaction:-
1. Adding oxygen:
C + O2 → CO2 (oxidation of carbon)
2. Adding an electronegative element:
Fe + S → FeS (oxidation of Iron)
3. Removing hydrogen:
H2S + Br2 → 2 HBr + S (oxidation of sulphide)
4. Removing electropositive elements:
2 KI + H2O2 → I2 + 2 KOH (oxidation of iodide)
An oxidising agent is used to carry out Oxidation. O2, S, Cl2, Br2, and H2O2 are oxidising agents used.
Reduction reactions:-
1. Adding hydrogen:
N2 + 3H2 → 2NH3 ( reduction of nitrogen)
2. Adding an electropositive element:
SnC2 + 2HgCl2 → SnCl4 + Hg2Cl2 ( reduction of mercuric chloride)
3. Removing oxygen
ZnO + C → Zn + CO (reduction of zinc oxide)
4. Removing an electronegative element
2FeCl3 + H2 → 2FeCl2 + 2HCl (reduction of ferric chloride)
Reducing agent is used to carry out Reduction. H2, HgCl2 and C are Reducing agents used above.
Remember:- The reactant, which goes for Oxidation, behaves as a reducing agent, whereas the reactant, which goes for Reduction, behaves as an oxidising agent.
What are Oxidising and Reducing Agents
The oxidising agent is the reactant that gains electrons and reduces to low valency. A reducing agent is a reactant that loses electrons and oxidises to high valency.
Some Oxidising Agents
The very strongest oxidising agent is Fluorine.
Examples of metals and non-metals include- MgO, CuO, CrO3, and P4O10.
Some Reducing Agents
All metals, including Na, Zn, Fe, Al as reducing agents.
Example of non-metals includes C, Hydrogen, S, P
Examples of hydracids are HCl, HBr, HI, H2S
Metallic hydrides examples are NaH, LiH, CaH2, etc.
The organic compound includes HCOOH as the reducing agent.
Conclusion:-
Oxidation and Reduction reaction plays a very vital role. The definition of a redox reaction occurs simultaneously. It has real-life uses in industry and manufacturing processes. The gaining of electrons is called Reduction, and the loss of electrons is called Oxidation. The oxidising and reducing capabilities of elements are termed the oxidation potential or the reduction potential of those elements. Redox reactions even occur in our body, and some chemical industries use redox reactions for various purposes.
