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iGCSE chemistry Section 2 lesson 4

iGCSE chemistry Section 2 lesson 4. Content. The iGCSE Chemistry course. Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3 Organic Chemistry Section 4 Physical Chemistry Section 5 Chemistry in Society. Content. Section 2

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iGCSE chemistry Section 2 lesson 4

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  1. iGCSE chemistrySection 2 lesson 4

  2. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3 Organic Chemistry Section 4 Physical Chemistry Section 5 Chemistry in Society

  3. Content Section 2 Chemistry of the Elements • The Periodic Table • Group 1 Elements • Group 7 Elements • Oxygen and Oxides • Hydrogen and Water • Reactivity Series • Tests for ions and gases

  4. f) Reactivity series 2.29 understand that metals can be arranged in a reactivity series based on the reactions of the metals and their compounds: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver and gold 2.30 describe how reactions with water and dilute acids can be used to deduce the following order of reactivity: potassium, sodium, lithium, calcium, magnesium, zinc, iron and copper 2.31 deduce the position of a metal within the reactivity series using displacement reactions between metals and their oxides, and between metals and their salts in aqueous solutions 2.32 understand oxidation and reduction as the addition and removal of oxygen respectively 2.33 understand the terms redox, oxidising agent, reducing agent 2.34 describe the conditions under which iron rusts 2.35 describe how the rusting of iron may be prevented by grease, oil, paint, plastic and galvanising 2.36 understand the sacrificial protection of iron in terms of the reactivity series Lesson 4 f) Reactivity Series

  5. What is the REACTIVITY SERIES?

  6. The REACTIVITY SERIES places metals in order of their reactivity based on how vigorously they react with water and dilute acids.

  7. The Reactivity Series ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold INCREASING REACTIVITY

  8. The Reactivity Series ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold INCREASING REACTIVITY { Very reactive

  9. The Reactivity Series ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold INCREASING REACTIVITY { Very reactive { Quite reactive

  10. The Reactivity Series ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold INCREASING REACTIVITY { Very reactive { Quite reactive { Not so reactive

  11. The Reactivity Series ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold INCREASING REACTIVITY { Very reactive { Quite reactive { Not so reactive { Unreactive

  12. Reaction with water ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold Very vigorous reaction with water, forming the hydroxide. Fizzes, and hydrogen is released. 2K(s) + 2H20(l) 2KOH(aq) + H2(g) 2Na(s) + 2H20(l) 2NaOH(aq) + H2(g) 2Li(s) + 2H20(l) 2LiOH(aq) + H2(g)

  13. Reaction with water ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold Slow reaction with cold water (very slow in the case of magnesium) to form the hydroxide. Bubbles of hydrogen gas will be seen. Ca(s) + 2H2O(l)  Ca(OH)2(aq) + H2(g) Mg(s) + 2H2O(l)  Mg(OH)2(aq) + H2(g)

  14. Reaction with water ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold Do not react with cold water, but will react with steam to form the oxide. Hydrogen gas is produced. Al(s) + 3H2O(l)  Al2O3(s) + 3H2(g) Zn(s) + H2O(l)  ZnO(s) + H2(g) Fe(s) + H2O(l)  FeO(s) + H2(g)

  15. Reaction with water ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold No reaction with water or steam

  16. Reaction with dilute acid ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold These elements react with acid in a very violent and dangerous manner. These experiments would not normally be attempted in the school laboratory. Examples: 2K(s) + 2HCl(aq)  2KCl(ag) + H2(g) 2Na(s) + H2SO4(aq)  Na2SO4(aq) + H2(g) Ca(s) + 2HNO3(aq)  Ca(NO3)2(aq) + H2(g)

  17. Reaction with dilute acid ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold These elements react reasonably well with acid, and the reactivity decreases as we go down the series. Examples: Mg(s) + 2HCl(aq)  MgCl2(ag) + H2(g) Zn(s) + H2SO4(aq)  ZnSO4(aq) + H2(g) Sn(s) + 2HNO3(aq)  Sn(NO3)2(aq) + H2(g)

  18. Reaction with dilute acid ELEMENT Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Tin Lead Copper Silver Gold No reaction with dilute acids

  19. Displacement reactions

  20. What is a DISPLACEMENT REACTION?

  21. A DISPLACEMENT REACTION is one in which a more reactive metal displaces a less reactive metal from a compound.

  22. In other words, a metal higher up in the reactivity series will ‘push out’ a metal that is lower in the series.

  23. “deduce the position of a metal within the reactivity series using displacement reactions between metals and their oxides, and between metals and their salts in aqueous solutions.”

  24. “deduce the position of a metal within the reactivity series using displacement reactions between metals and their oxides, and between metals and their salts in aqueous solutions.”

  25. Displacement reactions Magnesium ribbon fuse Iron plug Aluminium powder + iron oxide A very violent displacement reaction occurs

  26. Displacement reactions Magnesium ribbon fuse Iron plug Aluminium powder + iron oxide Aluminium + Iron oxide  Aluminium oxide + Iron

  27. Displacement reactions Magnesium ribbon fuse Iron plug Aluminium powder + iron oxide Aluminium + Iron oxide  Aluminium oxide + Iron Al(s) + FeO(s)  Al2O3(s) + Fe(s)

  28. “deduce the position of a metal within the reactivity series using displacement reactions between metals and their oxides, and between metals and their salts in aqueous solutions.”

  29. Displacement reactions Iron nail Copper deposit Copper sulphate solution Displacement reaction occurs Iron sulphate solution

  30. Displacement reactions A displacement reaction occurs because iron is higher than copper in the reactivity series Iron nail Copper deposit Copper sulphate solution Displacement reaction occurs Iron sulphate solution

  31. Displacement reactions A displacement reaction occurs because iron is higher than copper in the reactivity series Iron nail Copper deposit Copper sulphate solution Displacement reaction occurs Iron sulphate solution Copper sulphate + Iron  Iron sulphate + Copper

  32. Displacement reactions A displacement reaction occurs because iron is higher than copper in the reactivity series Iron nail Copper deposit Copper sulphate solution Displacement reaction occurs Iron sulphate solution CuSO4(aq) + Fe(s) FeSO4(aq) + Cu(s)

  33. Displacement reactions Will displacement reactions occur?

  34. Displacement reactions Will displacement reactions occur?

  35. Displacement reactions Will displacement reactions occur?

  36. Oxidation and Reduction Understand oxidation and reduction as the addition and removal of oxidation respectively

  37. Oxidation and Reduction Understand oxidation and reduction as the addition and removal of oxidation respectively • Oxidation may be defined in three ways: • Oxidation is the addition of oxygen to a substance • Oxidation is the removal of hydrogen from a substance • Oxidation is the loss of electrons from a substance

  38. Oxidation and Reduction Understand oxidation and reduction as the addition and removal of oxidation respectively Examples of oxidation: S(s) + O2(g) SO2(g) 2CO(g) + O2(g) 2CO2(g)

  39. Oxidation and Reduction Understand oxidation and reduction as the addition and removal of oxidation respectively • Reduction may be defined in three ways: • Reduction is the removal of oxygen from a substance • Reduction is the addition of hydrogen to a substance • Reduction is the gain of electrons by a substance

  40. Oxidation and Reduction Understand oxidation and reduction as the addition and removal of oxidation respectively Examples of reduction: 2Pb3O4(s) 6PbO(s) + O2(g) 2NaNO3(s) 2NaNO2(s) + O2(g)

  41. Oxidation and Reduction Understand the terms redox, oxidising agent, reducing agent

  42. Oxidation and Reduction Understand the terms redox, oxidising agent, reducing agent What is redox?

  43. Oxidation and Reduction Understand the terms redox, oxidising agent, reducing agent ? What is redox?

  44. In a redox reaction, both reduction and oxidation occur. For example, when hydrogen is passed over heated copper oxide, copper and water vapour are formed.

  45. Oxidation and Reduction Anhydrous copper sulphate Copper oxide Dry hydrogen Excess hydrogen HEAT

  46. In a redox reaction, both reduction and oxidation occur. The water vapour can be trapped by the anhydrous copper sulphate, turning it from white to blue. The excess hydrogen is burnt.

  47. In a redox reaction, both reduction and oxidation occur. CuO(s) + H2(g) Cu(s) + H2O(g) HEAT

  48. In a redox reaction, both reduction and oxidation occur. CuO(s) + H2(g) Cu(s) + H2O(g) OXIDATION HEAT

  49. In a redox reaction, both reduction and oxidation occur. CuO(s) + H2(g) Cu(s) + H2O(g) OXIDATION HEAT REDUCTION

  50. In a redox reaction, both reduction and oxidation occur. CuO(s) + H2(g) Cu(s) + H2O(g) OXIDATION HEAT REDOX REDUCTION

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