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Study the 6 Type of Chemical Reactions with Example

Chemical Reaction and its meaning-

A chemical reaction is when two or more than two chemical compounds or elements react to form some other entirely different chemical compound.Like

A + B -> C + D

In the above reaction the reactants A and B combine to form two different substances C and D which are the products.

For example

Cu + H2SO4 -> CuSO4 + H2

Chemical reactions are classified into 6 categories depending on the association between the reactants and the resultant products.

-> Combination reaction

-> Decomposition reaction

-> Displacement reaction

-> Redox reaction

-> Neutralization reaction

-> Dissociation reaction

Here we are going to discuss the 6 types of reactions in detail

Combination reaction

It is also called a synthesis reaction. In this type of reaction two or more reactants combine to form a different product.

A + B -> AB

It is also called a synthesis reaction. In this type of reaction two or more reactants combine to form a different product.

A + B ->AB

For example

MgO+ CO2→MgCO3


2CaO + 2H2O → 2Ca(OH)2

C + O2 → CO2

O2 + 2H2O → 2H2O2

Decomposition reaction

It is also called an analysis reaction. In this type of reaction a reactant breaks into two or more than two different products.
AB ->A + B

For example

2 H 2O2 → 2 H2O + O2

H2CO3 → H2O + CO2

CaCO3 → CaO + CO2

2 KClO3 → 2KCl + 3O2

Displacement reaction

A displacement reaction is when a component of one of the reactants is replaced by the other reactant.

If one of the reactants replaces the component of the other reactant it is called a single displacement reaction.

AB + C -> AC + B

For example

Zn + CuCl2 –> ZnCl2 + Cu

Mg + HCl –> MgCl2 + H2

Cu(s) + 2AgNO3(aq) -> 2 Ag(s) + Cu(NO3)2(aq)

If the reactants displace each other’s components mutually, it is called a double displacement reaction.

AB + CD -> AC + BD

For example

Na2CO3(aq) + 2HCl(aq) -> 2NaCl(aq) + H2CO3(aq)

NH4Cl(aq) + NaOH(aq) -> NaCl(aq) + NH4OH(aq)

Redox reactions

In redox reactions both oxidation and reduction take place simultaneously. Oxidation can be explained as any three of the following cases

• as addition of oxygen or

• addition of an electronegative element or

• removal of an electro positive element.

While, on the other hand, reduction is the absolute opposite of this.

Examples of oxidation and reduction reactions are

Fe2O3 + HCl → FeCl3 + H2O (oxidation of chlorine as hydrogen is removed)

Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(l) ( oxidation of aluminum [Al] and reduction of iron [Fe] )

Reduction involves addition of hydrogen.

In general oxidation is said to take place when there is a loss of electrons while reduction is said to take place when there is a gain of electrons.

Neutralization reactions

Neutralization reactions are the ones which take place between an acid and a base or alkali. Whenever an acid reacts with an alkali the result is the corresponding salt and water. Thus a neutralization reaction can be summarized as

HA + BOH -> AB + H2O

For example

HCl + NaOH –> NaCl + HOH

H 2SO4 + 2 NH 4OH –> (NH 4) 2SO4 + 2 HOH

2 NaOH + H 2CO3 –> N 2CO3 + 2 NaOH

Since there is always the formation of water in neutralization reactions they are also called ‘water forming reactions’

Dissociation reaction

Dissociation reaction is a form of decomposition reaction.

The difference between dissociation and decomposition reactions is that in decomposition reactions the reactant decomposes or breaks down into two or more elements or compounds, while in a dissociation reaction the reactant splits up into its ions.

Thus a dissociation reaction can be represented as

AB -> A+ + B-

For example

HCl -> H+ + Cl-

NaCl -> Na+ + Cl-

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Sarge Maisky

About Sarge Maisky

B. science, General Diploma in Education from Stanford university USA Sarge Maisky has written 250 articles on education and parenting.

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