Types_of_Chemical_Reactions_with_Examples.pptx

types of chemical reaction with examples

1. Types of Chemical Reactions With Examples | Grade 11 Science Presented by: Kip Aiza F. Gabawa

2. Learning Objectives • Define each type of chemical reaction. • Identify and classify reactions based on their characteristics. • Provide examples and balanced equations for each type. • Appreciate how these reactions occur in daily life.

3. What Are Chemical Reactions? • A chemical reaction occurs when one or more substances change into new substances. • It involves breaking and forming of chemical bonds. • Atoms are rearranged, conserving mass in the process.

4. Main Types of Chemical Reactions 1. Combination (Synthesis) Reaction 2. Decomposition Reaction 3. Single Replacement Reaction 4. Double Replacement Reaction 5. Combustion Reaction

5. 1. Combination (Synthesis) Reaction • Two or more reactants combine to form one product. General Formula: A + B → AB Example: 2H₂ + O₂ → 2H₂O • Common in forming compounds such as water or ammonia.

6. 2. Decomposition Reaction • One compound breaks down into two or more simpler substances. General Formula: AB → A + B Example: 2H₂O → 2H₂ + O₂ • Usually requires heat, light, or electricity to occur.

7. 3. Single Replacement Reaction • One element replaces another element in a compound. General Formula: A + BC → AC + B Example: Zn + 2HCl → ZnCl₂ + H₂ • Often occurs between metals and acids.

8. 4. Double Replacement Reaction • Ions in two compounds exchange places to form new compounds. General Formula: AB + CD → AD + CB Example: NaCl + AgNO₃ → NaNO₃ + AgCl • Common in precipitation and neutralization reactions.

9. 5. Combustion Reaction • A substance reacts rapidly with oxygen to produce heat and light. General Formula: Hydrocarbon + O₂ → CO₂ + H₂O Example: CH₄ + 2O₂ → CO₂ + 2H₂O • Commonly observed in burning fuels and respiration.

10. Visual Summary • Combination: A + B → AB • Decomposition: AB → A + B • Single Replacement: A + BC → AC + B • Double Replacement: AB + CD → AD + CB • Combustion: Hydrocarbon + O₂ → CO₂ + H₂O

11. Real-Life Applications • Combustion – car engines, cooking gas, and candles. • Decomposition – electrolysis of water, decay of organic matter. • Synthesis – formation of ammonia for fertilizers. • Replacement – rusting of iron, metal plating processes.

12. Balancing Chemical Equations • Ensures that the law of conservation of mass is followed. • Equal number of atoms of each element on both sides. • Example: 2H₂ + O₂ → 2H₂O is balanced.

13. Energy in Reactions • Exothermic: releases heat (e.g., combustion). • Endothermic: absorbs heat (e.g., photosynthesis). • Energy change depends on bond breaking and formation.

14. Importance of Classifying Reactions • Helps predict products of unknown reactions. • Aids in understanding chemical behavior of substances. • Useful in industries, medicine, and environmental studies.

15. Review Questions 1. What are the five main types of chemical reactions? 2. Which reaction type releases energy as heat and light? 3. Give one real-life example of a decomposition reaction. 4. What does balancing a chemical equation ensure? 5. Why is classification of reactions important in science?

16. Summary • Five main reaction types: Combination, Decomposition, Single Replacement, Double Replacement, Combustion. • Each type follows a distinct pattern and serves vital roles in nature and industry. • Understanding these helps explain many everyday processes around us.