Class 10 Science Chapter 1 PPT (46 Slides) – Chemical Reactions and Equations | USP Indore

Class 10 Science Chapter 1 PPT – Chemical Reactions and Equations | 46 Slides | USP Indore

Download the complete 46-slide illustrated PowerPoint presentation for Class 10 Science Chapter 1 – Chemical Reactions and Equations, prepared by Unique Study Point (USP), Indore. This PPT covers every concept, NCERT activity, type of reaction, chemical equation, and exercise of the chapter. Based on the CBSE NCERT syllabus (session 2026-27).

Complete Topic Coverage — 46 Slides

🔬 Part 1 — Signs of a Chemical Reaction (Slides 1–2)

• How do we know a chemical reaction has occurred? — 4 signs to look for
• Change iColor—Ironon nails in CuSO₄ solution (blue → pale green)
• Change in State — Candle wax (solid → liquid → gas + CO₂); physical vs chemical change
• Evolution of Gas — Zinc granules in dilute H₂SO₄ → H₂ gas
• Change in Temperature — Exothermic (gets HOT) vs Endothermic (gets COLD)

🎆 Part 2 — Activity 1.1: Burning Magnesium Ribbon (Slide 3)

• Magnesium ribbon cleaned with sandpaper → held in tongs → burned over spirit lamp
• ⁣ bservation: Dazzling white flame; white powder (MgO) collected on watch glass
• Equation: 2Mg + O₂ → 2MgO (balanced; atom count verified)
• This is a Combination + Exothermic reaction; Mg is OXIDISED (gains oxygen)
• Safety note: Keep Mg ribbon away from eyes; wear eye protection

⚖️ Part 3 — Chemical Equations and Balancing (Slides 4–8)

• ⁣ hat is a chemical equation? Reactants (LHS) → Products (RHS)
• Skeletal equation (unbalanced) . balanced equation—differencece explained
• Law of Conservation of Mass: Mass is NEVER created or destroyed; atoms must be equal on both sides
• Balancing Rule 1: Change COEFFICIENTS (numbers before formula) to balance
• Balancing Rule 2: NEVER change subscripts insida formula—4H₂O₂O is OK; H₂O₄ is WRONG!
• Example: Mg + O₂ → MgO (unbalanced) → 2Mg + O₂ → 2MgO (balanced)
• State symbols: (s) solid, (l) liquid, (g) gas, (aq) aqueous
• In-chapter Q1: Why clean Mg ribbon with sandpaper before burning?
• In-chapter Q2: Balance equations — H₂ + Cl₂ → 2HCl; 3BaCl₂ + Al₂(SO₄)₃ → 3BaSO₄ + 2AlCl₃; 2Na + 2H₂O → 2NaOH + H₂
• In-chapter Q3: Write equations with state symbols — BaCl₂(aq) + Na₂SO₄(aq) → BaSO₄(s)↓ + 2NaCl(aq); NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

🧪 Part 4 — Types of Chemical Reactions (Slides 9–25)

1. Combination Reaction — Activity 1.4 (Slide 10)

• ⁣ efinition: Two or more substances combine → ONE single new product (A + B → AB)
• CaO(s) + H₂O(l) → Ca(OH)₂(aq) + Heat Quicklime e + Water → Slaked lime
• Exothermic: Beaker gets very HOT; large amount of heat released
• ⁣ ther examples: C(s) + O₂(g) → CO₂(g); 2H₂(g) + O₂(g) → 2H₂O(l)

2. Decomposition Reaction — Activities 1.5, 1.6, 1.7 (Slides 11–15)

• Definition: ONE reactant breaks down into two or more simpler products
• Activity 1.5 — Thermal Decomposition (FerrouSulfate Heating):): 2FeSO₄(s→ [Heat] →]→ Fe₂O₃(s) + SO₂(g) + SO₃(g); green crystals → reddish-brown powder; pungent smell of SO₂/SO₃
• Mini example: CaCO→ [Heat] →]→ CaO + CO₂ (used in cement industry!)
• Activity 1.6 — Lead Nitrate heating: 2Pb(NO₃)₂(s→ [Heat] →]→ 2PbO(s) + 4NO₂(g) + O₂(g); brown fumes of NO₂; crackling sound
• Activity 1—Electrolysisis of Water (Electrolytic Decomposition): 2H₂O(l→ [Electricity] →]→ 2H₂(g) + O₂(g); H₂:O₂ volume ratio = 2:1 always; burning splint near H₂ → burns with POP; glowing splint near O₂ → relights
• Activity 1—Photolysisis (Silver Chloride): 2AgCl(s→ [Sunlight] →]→ 2Ag(s) + Cl₂(g); white AgCl turns grey in sunlight

3. Displacement Reaction — Activity 1.9 (Slide 20)

• Definition: More reactive element displaces less reactive element from its salt solution
• Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s); iron nail coated with BROWN copper deposit; blue solution fades (Cu²⁺ used up); light green FeSO₄ solution forms
• Iron displaces copper because Fe is MORE REACTIVE than Cu
• ⁣ ther examples: Zn + CuSO₄ → ZnSO₄ + Cu; Pb + CuCl₂ → PbCl₂ + Cu

4. Double Displacement Reaction — Activity 1.10 (Slide 23)

• ⁣ efinition: Two different atoms/groups (ions) exchange between two compounds (AB + CD → AD + CB)
• Na₂SO₄(aq) + BaCl₂(aq) → BaSO₄(s)↓ + 2NaCl(aq); white precipitate of BaSO₄ forms instantly!
• Reaction producing INSOLUBLE product = PRECIPITATION REACTION

5. Oxidation and Reduction (Redox) — Activity 1.11 (Slide 25)

• Activity 1.11: Cu heated in air → black CuO forms (2Cu + O₂ → 2CuO); H₂ gas over hot CuO → brown Cu appears again (CuO + H₂ → Cu + H₂O)
• OXIDATION = Gain of oxygen OR loss of hydrogen
• REDUCTION = Loss of oxygen OR gain of hydrogen
• REDOX: Oxidatioand reductionon occur SIMULTANEOUSLY in the same reaction
• CuO + H₂ → Cu + H₂O: H₂ gains oxygen (OXIDISED); CuO loses oxygen (REDUCED)

🦀 Part 5 — Effects of Oxidation: Corrosion and Rancidity (Slides 28–33)

• ⁣⁣ rrosion: When a metal is attacked by substances around it (moisture, acid, gases)
• Iron Rusting: Iron + O₂ + H₂O → Fe₂O₃·xH₂O (rust); reddish-brown coating; damages bridges, ships, cars, iron railings — HUGE economic loss
• Silver Tarnishing: Silver + H₂S (from air) → Ag₂S (black coating on jewellery and silverware)
• Copper Green Patina: Copper + CO₂ + H₂O → Basic Copper Carbonate (green patina on statues, pipes, utensils)
• Rancidity: Oxidation of fats and oils → bad smell and taste (rancid food)
• Prevention: Antioxidants added; nitrogen gas flushing in chips packetsrefrigeration, andn; airtight containers

📝 Part 6 — In-Chapter and Exercise Questions (Slides 34–45)

• Glossary slide: All key ter—Reactant,t, Product, Skeletal Equation, Balanced Equation, Combination, Decomposition, Exothermic, Endothermic, Displacement, Precipitate, Corrosion, Rancidity
• Exercise Q1: What is a chemical equation? Why should it be balanced?
• Exercise Q2: What is a balanced chemical equation? Why should chemical equations be balanced?
• Exercise Q3: Write balanced equations for — (a) hydrogen + chlorine → hydrogen chloride; (b) barium chloride + aluminium sulphate → barium sulphate + aluminium chloride; (c) sodium + water → sodium hydroxide + hydrogen
• Exercise Q4: Write balanced equations with state symbols for—(a) dilute H₂SO₄ + zinc → zinc sulphate + hydrogen; (b) NaOH + H₂SO₄ → Na₂SO₄ + H₂O; (c) NaCl + AgNO₃ → AgCl↓ + NaNO₃
• Exercise Q5: What is a reactant? Product? Give examples.
• Exercise Q6: Balance equations — (a) HNO₃ + Ca(OH)₂ → Ca(NO₃)₂ + H₂O; (b) NaOH + H₂SO₄ → Na₂SO₄ + H₂O; (c) NaCl + AgNO₃ → AgCl↓ + NaNO₃; (d) BaCl₂ + H₂SO₄ → BaSO₄↓ + HCl
• Exercise Q7: Identify types of reactio—combination,n, decomposition, displacement, double displacement, redox

🎉 Slide 46 — Group Activity + Chapter Summary

• Group Activity: K₂SO₄, NH₄NO₃CuSO₄, and₄, irofilings aregs added to wat—whichch beakers get HOT (exothermic)? Which gets COLD (endothermic)?
• Chapter Summary: Chemical equations represent reactions using formulas. Always balance equations (Law of Conservation of Mass). 5 types: Combination, Decomposition, Displacement, Double Displacement, Redox; Exothermic = heat out; Endothermic = energy in; Corrosion = metal attacked; Rancidity = fat/oil oxidized.

All NCERT Activities Covered in This PPT

• ⁣ Activity 1.1 — Burning Magnesium Ribbon
• ✅ Activity 1.4 — Combination Reaction: CaO + H₂(Quicklime e + Water)
• ⁣ Activity 1.5 — Thermal Decomposition: Ferrous Sulfate Heating
• ⁣ Activity 1.6 — Lead Nitrate thermal decomposition (brown NO₂ fumes)
• ⁣ Activity 1.7 — Electrolysis of Water (H₂:O₂ = 2:1)
• ⁣ Activity 1.8 — Photolysis of Silver Chloride (AgCl → Ag + Cl₂)
• ⁣ Activity 1.9 — Displacement Reaction: Iron nail in CuSO₄ solution
• ✅ Activity 1.10 — Double Displacement: Na₂SO₄ + BaCl₂ → BaSO₄↓
• ✅ Activity 1.11 — Oxidation and Reduction: CuO + H₂ → Cu + H₂O (Redox)

Key Features of This Presentation

• ✅ 46 slides — the most detailed Class 10 Chapter 1 Science PPT available
• ⁣ All 9 NCERT Activities (1.1 to 1.11) covered with lab diagrams
• ✅ All 5 types of reactions explained with equations and real examples
• ✅ Balancing equations — step-by-step with atom count verification
• ⁣ All Exercise questions (Q1 to Q7) solved and explained
• ⁣ Corrosion and Rancidity with prevention methods
• ⁣ Key Terms Glossary slide for quick revision
• ⁣ Chapter Summary on final slide
• ⁣ Prepared as per CBSE NCERT Class 10 Science Syllabus 2026-27

Important Chemical Equations Covered

• 2Mg + O₂ → 2MgO (Burning Magnesium — Combination + Exothermic)
• CaO + H₂O → Ca(OH)₂ + Hea(Quicklime e + Water — Combination + Exothermic)
• 2FeSO→ [Heat] →]→ Fe₂O₃ + SO₂ + SO₃ (Thermal Decomposition)
• CaCO→ [Heat] →]→ CaO + CO₂ (Thermal Decomposition — cement industry)
• 2H₂→ [Electricity] →]→ 2H₂ + O₂ (Electrolytic Decomposition)
• 2AgC→ [Sunlight] →]→ 2Ag + Cl₂ (Photolysis)
• Fe + CuSO₄ → FeSO₄ + Cu (Displacement)
• Na₂SO₄ + BaCl₂ → BaSO₄↓ + 2NaCl (Double Displacement / Precipitation)
• CuO + H₂ → Cu + H₂O (Redox — Oxidation + Reduction simultaneously)
• Ba(OH)₂ + 2NH₄Cl → BaCl₂ + 2NH₃↑ + 2H₂O (Endothermic)

Important FAQs — Class 10 Science Chapter 1

Q. What are the signs that a chemical reaction has occurred?
Ans. Four signs indicate a chemical reaction: (1) Change in color—e.g., an iron nail turns brown in CuSO₄ solution; (2) Change in state—e.g., candle wax melts and burns to CO₂ gas; (3) Evolution of gas—e.g., H₂ gas released when zinc reacts with dilute H₂SO₄; (4) Change in temperature—exothermic reactions release heat; endothermic reactions absorb heat.

Q. Why should a chemical equation be balanced?
Ans. A chemical equation must be balanced to follow the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction. The total number of atoms of each element must be equal on both sides (reactants and products).

Q. What are the 5 types of chemical reactions?
Ans. The five types are: (1) Combination Reaction — A + B → AB; (2) Decomposition Reaction — AB → A + B; (3) Displacement Reaction — A + BC → AC + B (more reactive A displaces B); (4) Double Displacement Reaction — AB + CD → AD + CB (ions exchange); (5) Oxidation-Reduction (Redox) Reaction — oxidation and reduction occur simultaneously.

Q. What is the difference between exothermic and endothermic reactions?
Ans. Exothermic reactions release heat energy to the surroundings—the reaction mixture gets HOT (e.g., CaO + H₂O → Ca(OH)₂ + Heat). Endothermic reactions absorb heat energy from the surroundings—the reaction mixture gets COLD (e.g., Ba(OH)₂ + 2NH₄Cl → BaCl₂ + 2NH₃ + 2H₂O).

Q. What is a redox reaction? Give an example.
Ans. A redox reaction is one in which both oxidation and reduction occur simultaneously. Oxidation = gain of oxygen or loss of hydrogen. Reduction = loss of oxygen or gain of hydrogen. Example: CuO + H₂ → Cu + H₂O. Here, H₂ gains oxygen (oxidized), and CuO loses oxygen (reduced). Both happen in the same reaction.

Q. What is the difference between corrosion and rancidity?
Ans. Corrosion is the process in which metals are attacked by substances around them (moisture, acids, gases), resulting in their gradual deterioration. Examples: rusting of iron (Fe₂O₃·xH₂O), tarnishing of silver (Ag₂S), green patina on copper. Rancidity is the oxidation of fats and oils in food, causing bad smell and taste. Prevention includes using antioxidants, nitrogen gas flushing, and airtight containers.

Q. Why is the volume of H₂ always double that of O₂ in electrolysis of water?
Ans. In electrolysis of water: 2H₂O → 2H₂ + O₂. According to this equation, for every 1 molecule of O₂ produced, 2 molecules of H₂ are produced. So H₂:O₂ volume ratio is always 2:1. H₂ collects at the cathode (−) and O₂ at the anode.

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