How Many Types of Chemical Reactions are There

Introduction

It is possible to categorise all chemical reactions into eight groups. A thorough understanding of these kinds of reactions is necessary to be able to recognise the byproducts of unknown processes. The eight basic types of chemical processes are combination, decomposition, single-displacement, double-displacement, combustion, precipitation, neutralisation and redox reaction. Let's learn about all these reactions in little detail.

What is a Chemical Reaction

chemical reaction, often known as the conversion of one or more chemicals (sometimes referred to as reactants) into one or more other compounds (the products). The atoms that make up the reactants of a chemical reaction are rearranged to create different products.

An essential aspect of life itself, as well as technology and civilization, are chemical reactions. A few examples of prehistoric operations that included chemical reactions were the burning of fuels, the smelting of iron, the production of glass and pottery, the brewing of beer and wine, and the production of cheese. Chemical reactions are abundant in the Earth's geology, atmosphere, oceans, and a vast range of complicated processes that occur in all biological systems.

Physical changes and chemical reactions must be differentiated. State transitions, such as ice melting into water and water evaporating into vapour, are examples of physical changes. If a material undergoes a physical change, its chemical identity will not change, but its physical attributes will. Water (H2O) is a substance that has two hydrogen atoms and one oxygen atom in each molecule, regardless of its physical condition. However, when water, whether it be frozen, liquid, or vapour, comes into contact with sodium metal (Na), the atoms are rearranged to create molecular hydrogen (H2) and sodium hydroxide (NaOH). We can infer a chemical change or reaction from this.

• Physical change: When a change in a substance's size or shape, which is often reversible, occurs. Examples of physical change include freezing a liquid, melting a candle, smashing a can, and shredding paper.

• Chemical change: A chemical change occurs when a material's chemical property changes. Examples of such qualities are density change, temperature change, energy change, etc. It is frequently referred to as a chemical reaction. A chemical change can occur during combustion, corrosion, fermentation, and other processes.

Properties Shown by a Chemical Reaction

• When two or more molecules combine and create a new product, a chemical reaction takes place(s).

• substances that combine to create a brand-new substance termed a reactant. and the substances that resulted from the reaction between the reactants are referred to as the product.

• In a chemical reaction, the physical change—such as the evolution of heat, change in colour, etc.—must precede the chemical change.

• No atom is generated or destroyed, only a new product is formed when two atoms, ions, or molecules of reactants interact to break existing bonds and make new ones.

• Pressure, temperature, and the concentration of the reactants are only a few of the variables that affect the reaction rate.

Types of Chemical Reactions

1. Combination reaction

• When two or more reactants combine to produce a single product, this is referred to as a combination reaction.

• It is expressed as

\begin{equation}

X+Y \rightarrow X Y

\end{equation}

• Combination reactions are another name for synthesis reactions.

• Combination reaction example

\begin{equation}

2 \mathrm{Na}+\mathrm{Cl}_2 \rightarrow 2 \mathrm{NaCl}

\end{equation}

2. Decomposition reaction

• A decomposition reaction is one in which a single chemical splits into two or simpler compounds.

• It is expressed as

\begin{equation}

X Y \rightarrow X+Y

\end{equation

• Reverse of the combination reaction is the decomposition reaction.

• Decomposition reaction example

\begin{equation}

\mathrm{CaCO}_3 \rightarrow \mathrm{CaO}+\mathrm{CO}_2

\end{equation}

• A thermal breakdown process is one in which a chemical breaks down as a result of heating.

3. Single-displacement reaction

• A chemical transformation in which one element is replaced by a more reactive one after leaving its aqueous salt solution.

• It has the following form

\begin{equation}

X+Y Z \rightarrow X Z+Y

\end{equation}

• Another name of this reaction is substitution reaction.

• Displacement reaction example

\begin{equation}

\mathrm{Zn}+\mathrm{CuSO}_4 \rightarrow \mathrm{ZnSO}_4+\mathrm{Cu}

\end{equation}

4. Double-displacement reaction

• A double displacement reaction is a chemical process in which ions are swapped between two reactants to create a new molecule.

• It looks as

\begin{equation}

X Y+Z A \rightarrow X Z+Y A

\end{equation}

• Another name of this reaction is metathesis reaction.

• Double displacement reaction example

\begin{equation}

\mathrm{BaCl}_2+\mathrm{Na}_2 \mathrm{SO}_4 \rightarrow \mathrm{BaSO}_4+2 \mathrm{NaCl}

\end{equation}

5. Combustion reaction

A fuel and an oxidant engage in a chemical process known as a combustion to create a byproduct known as an ad oxidised product. An oxidizer is a chemical fuel, like oxygen, that is needed to burn. Typically, carbon dioxide, water, and heat are produced when a hydrocarbon and oxygen combine.

An example of a combustion reaction is:

\begin{equation}

\mathrm{CH}_4(\mathrm{~g})+2 \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{g})+\text { Heat }

\end{equation}

6. Precipitation reaction

• A precipitation reaction is a name for a chemical reaction that results in the creation of an insoluble product.

• Despite the liquid nature of the reactants, the end product is insoluble and separates as a solid.

• The chemical equation that describes a chemical change is sufficient for reactions in solutions, however, the standard molecular equation has distinct representations for reactions of ionic substances in an aqueous solution (water).

• A molecular equation may rule out the formulae of the ions that are the actual reactants and products while indicating the formulas of reactants and products that aren't there.

• If the part of the molecular equation that is really present as dissociated ions is stated in the form of their ions, the resultant equation is an ionic equation.

Example:

\begin{equation}

\mathrm{AgNO}_{3(a q)}+\mathrm{KCl}_{(a q)} \leftrightarrow \quad \mathrm{AgCl}+\mathrm{KNO}_{3(a q)}

\end{equation}

7. Neutralisation reaction

An acid and a base will react to produce salt and water in a neutralisation process. The interaction of OH– and H+ ions results in the production of water molecules. When a strong base and a strong acid combine to neutralise one another, the final products must have a pH of 7. Think about the neutralisation reaction between sodium hydroxide (NaOH) and hydrochloric acid (HCl), which results in sodium chloride (common salt) and water.

8. Redox reaction

Redox reactions are those chemical processes in which oxidation and reduction occur concurrently. While reduction involves the addition of hydrogen, oxidation involves the addition of oxygen (or removal of oxygen).

An example of a redox reaction is the interaction of copper oxide with hydrogen. In this process, copper oxide has experienced reduction by the removal of oxygen, whereas hydrogen has undergone oxidation by obtaining oxygen atoms.

Conclusion

With this, we have ended with learning almost all types of basic chemical reactions with their suitable examples. We have also learned about a few properties exhibited by these chemical reactions in common. After reading this article we can easily differentiate between various chemical reactions.