Class 10 Physical Science
Chapter 2: Chemical Equations
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🗺️ Interactive Mind Map 1: Chemical Equations
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Choose any coloured branch above. Its explanation and example will appear here.🧠 Interactive Mind Map 2: Types of Reactions
📚 Student-Ready Notes
1. What is a chemical reaction?
A chemical reaction is a process in which one or more substances change into new substances with different properties.2. What is a chemical equation?
A chemical equation represents a chemical reaction using chemical symbols and formulae.- Reactants: Substances that take part in a reaction; written on the left.
- Products: New substances formed; written on the right.
- Arrow (→): Indicates the direction of the reaction.
- Coefficients: Numbers placed before formulae to balance atoms.
- State symbols: (s) solid, (l) liquid, (g) gas, (aq) aqueous solution.
3. Balanced and unbalanced equations
A balanced equation has the same number of atoms of each element on both sides. It follows the law of conservation of mass.4. Steps to balance a chemical equation
- Write the correct formulae of all reactants and products.
- Count atoms of every element on both sides.
- Add suitable coefficients to balance the atoms.
- Recount all atoms and reduce coefficients to the smallest whole-number ratio.
- Include state symbols and reaction conditions where required.
5. Types of chemical reactions
| Type | Example |
|---|---|
| Combination | CaO + H₂O → Ca(OH)₂ |
| Decomposition | CaCO₃ → CaO + CO₂ (on heating) |
| Displacement | Zn + CuSO₄ → ZnSO₄ + Cu |
| Double displacement | AgNO₃ + NaCl → AgCl + NaNO₃ |
| Combustion / oxidation | CH₄ + 2O₂ → CO₂ + 2H₂O |
These equations are balanced. In the decomposition example, heating is required. Silver chloride forms a precipitate in the double-displacement example.
6. Exothermic and endothermic reactions
- Exothermic: Releases energy to the surroundings. Example: combustion of fuels.
- Endothermic: Absorbs energy from the surroundings. Example: thermal decomposition of calcium carbonate.
7. Oxidation and reduction
- Oxidation: In classical examples, gain of oxygen or loss of hydrogen; in electron terms, loss of electrons.
- Reduction: In classical examples, loss of oxygen or gain of hydrogen; in electron terms, gain of electrons.
- Redox reaction: Oxidation and reduction occur together.
CuO is reduced to Cu, while H₂ is oxidised to H₂O.
8. Corrosion and rancidity
- Corrosion: Gradual damage to a metal by its environment. Rusting of iron requires oxygen and moisture.
- Prevention: Painting, oiling, greasing, galvanising or suitable protective coatings.
- Rancidity: Oxidation of fats and oils that causes unpleasant smell and taste.
- Prevention: Airtight storage, refrigeration, antioxidants and limiting exposure to air.
9. Important observations
- Evolution of gas or formation of a precipitate may indicate a chemical reaction.
- Colour change and temperature change may also indicate a reaction.
- Symbols such as Δ above an arrow indicate heating; sunlight or electricity may be shown as reaction conditions.
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