Types of chemical reactions class 10th CBSE with types of each reaction

Types of chemical reactions class 10th CBSE with types of each reaction 

Chemical reactions are the processes in which chemicals react to form new chemicals with different properties. In other words, we can say that a chemical reaction is a process where reactants are transformed into 2 products. 

Chemical reactions are constantly occurring in the world around us; everything from the rusting of an iron nail to the digestion of food is an example of a chemical reaction. Chemistry is an attempt to classify and understand these reactions in a better way.

So, types of chemical reactions are as follows:

1. Combination Reaction 

It can be defined as a chemical reaction in which two or more substances combine to form a single substance under suitable conditions. Combination reactions are also known as synthesis, because in these reactions new substances are synthesized. the simplest equation of a combination reaction is illustrated below-

                   A+B ➡️ AB

Some of the common types of combination reactions are described below-

a) Reaction between two or more elements

b) Reaction between elements and compounds

c) Reaction between two compounds

 

2. Decomposition Reaction

A decomposition reaction is the opposite of a combination reaction. During the decomposition reaction, a complex compound break down into multiple simpler compounds.

                   A ➡️ B+C

most of the decomposition reactions are endothermic as they require energy in the form of heat, light or electricity. Absorption of energy causes the breaking of the bonds present in the reacting substance, which decomposes to give the product.

Some of the common types of decomposition reactions are provided below-

a) Thermal decomposition: some compounds break down when heated, forming two or more products from one reactant. This type of reaction is called thermal decomposition or thermolysis.

b) When decomposition is carried out with the help of electricity it is called electrolysis.

c) When decomposition is carried out in the presence of light, it is called as photochemical decomposition

3. Single Displacement Reaction

Displacement reaction is a chemical reaction in which a more reactive element displaces a less reactive element from its compound. Displacement reaction is also known as substitution reaction or single displacement/ replacement reaction. 

                    A+BC ➡️ AC+B

displacement reaction can take place only when 'A' is more reactive than 'B'. If 'B' is more reactive than 'A', then 'A' cannot displace 'C' from 'BC' and displacement reaction cannot take place.

Metals above hydrogen in the reactivity series can displace hydrogen from dilute acids.

For example, metals such as potassium ,sodium magnesium, zinc, e.t.c., react more vigorously with dilute acid to form metal salts and hydrogen gas.

4. Double Displacement Reaction

Double Displacement reactions are chemical reactions in which the compounds react to form two different compounds by the mutual exchange of ions.

               AB+CD ➡️ AD+CB

When the solution of barium chloride reacts with the solution of sodium sulphate, a white precipitate of barium sulphate is formed along with sodium chloride.

Double displacement reactions in which precipitate are formed are also known as precipitation reactions.

There are various examples of double displacement reactions happening around us.

One of the commonly observed double displacement reactions is the erosion of marble due to acid rain. The oxides of nitrogen form nitric acid when they react with water. The resulting nitric acid present in the acid rain reacts with marble, thereby resulting in a double displacement reaction. Calcium carbonate present in the limestone of marble gets converted into calcium nitrate along with the evolution of carbon dioxide and water which results in the loss of artwork.

5. Redox reaction

Redox reactions are everywhere! your body uses redox reactions to convert food and oxygen to energy, water and carbon dioxide, which you then exhale. the batteries in your electronics also rely on redox reactions.

As the name suggests, a redox reaction is one in which oxidation and reduction takes place simultaneously. In order to understand such reactions, we need to know about oxidation and reduction processes.

a) Oxidation is defined as a process that involves the gain of oxygen or removal of hydrogen.

b) Reduction is defined as a process that involves the loss of oxygen or addition of hydrogen.

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