Class 10 Science Chapter 1 Notes Chemical Reactions and Equations We have provided class 10 science revision notes for Chapter 1 Chemical Reactions and Equations these notes give you a clear and in-depth explanation of the chapter so that class 10 students can easily understand the chapter theory concept.
| Class | Class 10 |
| Subject | Science |
| Chapter | Chapter 1 |
| Chapter Name | Chemical Reactions and Equations |
| Category | CBSE Notes |
Class 10 Science Chapter 1 Notes Chemical Reactions and Equations This note contains CBSE Key Notes, CBSE Revision Notes, and diagrams of the complete Chapter 1 Chemical Reactions and Equations of Science class 10, To score good marks in the board exam it is necessary to revise these notes, Here notes are given with detailed explanation so that it helps students to understand the chapter in a better way. Chemical Reactions and Equations Notes Those Students who are preparing for their Class 10 Board exams must go through NCERT notes for Class 10 Science Chapter 1 Notes Chemical Reactions and Equations Notes.
Class 10 Science Chapter 1 Notes Chemical Reactions and Equations
Chemical Reaction
The process in which new substances with new properties are formed is called Chemical Reaction.
- The substances which take part in chemical reaction are called Reactants.
- The substances which are formed in a chemical reaction are called Products.
Examples
(i) Digestion of food
(ii) Respiration
(iii) Rusting of iron
(iv) Burning of Magnesium ribbon
(v) Formation of curd
Chemical reaction involves :
- Change in state
- Change in colour
- Change in temperature
- Evolution of gas
Chemical Equation
A chemical reaction can be represented by chemical equation. It involves uses of symbol of elements or chemical formula of reactant and product with mention of physical state.
e.g. Magnesium is burnt in air to form Magnesium oxide.
2Mg + O2 → 2MgO
Types Of Chemical Reactions
1. Combination Reaction: The reaction in which two or more reactants combine to form a single product.
A+B→C
(i) Burning of coal
C(s) + O2 (g) → CO₂ (g)
(ii) Formation of water
2H₂ (g) + O2 (g) → 2H₂O(l)
(iii) CaO(s) + H₂O(l) → Ca(OH)2(aq)
Exothermic Reactions: Reaction in which heat is released along with formation of products.
e.g.,
(i) Burning of natural gas
CH4 (g) + O2 (g) → CO2 (g) + 2H2O(g) + Heat
(ii) Respiration is also an exothermic reaction.
C6H12O6 (aq) + 6O2 (g) → 6CO2 (g) + 6H2O (l) + energy
2. Decomposition Reaction: Reactions in which one compound decomposes in two or more compounds or elements are known as Decomposition Reaction.
A decomposition reaction is just the opposite of combination reaction.
A → B + C
Thermal decomposition : When decomposition is carried out by heating.
Electrolytic Decomposition : When decomposition is carried out by passing electricity.
Photolytic Decomposition : When decomposition is carried out in presence of sunlight.
The decomposition reactions are mostly endothermic in nature. Energy in the form of heat, light or electricity is generally absorbed in these reactions
e.g.,
Silver chloride turns grey on exposure to sunlight
* Above reaction is used in black and white photography.
Endothermic Reactions : The reactions which require energy in the form of heat, light or electricity to break reactants are called endothermic reactions.
3. Displacement Reaction: The chemical reaction in which more reactive element displaces less reactive element from its salt solution.
e.g., Fe (s) + CuSO4 (aq) → FeSO4(aq) + Cu (s)
The iron nail becomes brownish in colour by deposition of Cu and blue colour of CuSO4 changes to dirty green colour due to formation of FeSO4.
Zn + CuSO4 → ZnSO4 + Cu
Zn is more reactive than copper.
4. Double Displacement Reaction : A reaction in which new compounds are formed by mutual exchange of ions between two compounds.
e.g., Na2SO4(aq) + BaCl2 (aq) → BaSO4 (s) + 2NaCl (aq)
white precipitate of BaSO4 is formed, so it is also called precipitation reaction.
Note: All double displacement reactions are not precipitation reactions.
Oxidation and Reduction
Oxidation
(i) The addition of oxygen to reactant.
(ii) The removal of hydrogen from a reactant.
e.g., C + O2 → CO2
Reduction
(i) The addition of hydrogen to reactant.
(ii) The removal of oxygen from a reactant.
In this reaction CuO is reduced to Cu and H2 is oxidized to H2O. So, oxidation and reduction taking place together is redox reaction.
Effects of Oxidation in Daily Life
Corrosion
- When a metal is exposed to moisture, air, acid etc. for some time, a layer of hydrated oxide is formed which weakens the metal and hence metal is said to be corroded.
- Rusting of iron, black coating on silver and green coating on copper are examples of corrosion
- Corrosion can be prevented by galvanization, electroplating or by applying paints.
Rancidity
The oxidation of fats and oils when exposed to air is known as rancidity. It leads to bad smell and bad taste of food.
Methods to Prevent Rancidity
- By adding antioxidants
- Keeping food in air tight containers
- Replacing air by nitrogen
- Refrigeration
Class 10 science notes
- Chapter 1 – Chemical Reactions and Equations
- Chapter 2 – Acids, Bases, and Salts
- Chapter 3 – Metals and Non-metals
- Chapter 4 – Carbon and Its Compounds
- Chapter 5 – Periodic Classification of Elements
- Chapter 6 – Life Processes
- Chapter 7 – Control and Coordination
- Chapter 8 – How do Organisms Reproduce?
- Chapter 9 – Heredity and Evolution
- Chapter 10 – Light Reflection and Refraction
- Chapter 11 – Human Eye and Colourful World
- Chapter 12 – Electricity
- Chapter 13 – Magnetic Effects of Electric Current
- Chapter 14 – Sources of Energy
- Chapter 15 – Our Environment
- Chapter 16 – Management of Natural Resources
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Class 10 Chemical Reactions and Equations Notes
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