Any chemical reaction which involves the transfer of electrons between any two participating species can be referred to as a redox reaction. These reactions can be found everywhere – From the batteries in electronic devices to the simple conversion of food into energy in the human body. Some basic information on the types of Oxidation-Reduction reactions can be found in this article.
When a substance undergoes combustion, it is basically undergoing a reaction alongside atmospheric oxygen to give rise to products that contain oxygen. These types of oxidation reduction reactions are typically accompanied by a release of energy.
An example of a combustion reaction would be the combustion of octane, a component of gasoline. This reaction can be written as:
2C8H18 + 25O2 → 16CO2 + 18H2O
In these types of oxidation reduction reactions, one single reactant undergoes both oxidation and reduction, yielding two different products. Disproportionation reactions are also referred to as autooxidation reactions.
An example of a disproportionation reaction is the hypochlorite ion undergoing disproportionation, which can be given by the following reaction:
3ClO- → ClO3- + 2Cl-
This reaction is also an example of anionic reactants undergoing a redox reaction. Cations and anions are ions that are positively and negatively charged respectively.
Single Replacement Reaction
This reaction describes the switching of places of two elements in a given compound. Single replacement reactions are also referred to as single displacement reactions.
An example of a single replacement reaction would be a reaction between zinc and hydrochloric acid. The reaction can be written as follows:
Zn + 2HCl → ZnCl2 + H2
To learn about the difference between exothermic reactions like combustion reactions and endothermic reactions, visit: