Chemistry for 14 -16 year olds: Metals and their compounds.

Slide 1 : 1 GCSE Questions and Answers Inorganic: Metal Chemistry Remember that you can search using “edit”! 6 consecutive papers: 2002-7 You can find a video-cast lesson on this here

Slide 2 : 2 POTASSIUM SODIUM LITHIUM CALCIUM MAGNESIUM ALUMINIUM ZINC IRON LEAD COPPER Displacement Reactions Copper + Iron ? Copper + Iron Sulphate Sulphate

Slide 3 : Zinc + Copper Sulphate ………… + ………... Copper Zinc Sulphate Magnesium + Iron oxide ………..…….. + …………...

Slide 4 : 4

Slide 5 : 5

Slide 6 : 6 AB(aq) + CD(aq) ? AD(s) + CB(aq)   AgNO3(aq) + NaCl(aq) ? AgCl(s) + NaNO3(aq)     CuSO4(aq) + 2NaOH(aq) ? Cu(OH)2(s) + Na2SO4(aq)     Pb(NO3)2 (aq) + Na2CO3 (aq) ? PbCO3(s) + 2NaNO3(aq)     FeSO4(aq) + 2NaOH(aq) ? Fe(OH)2(s) + Na2SO4(aq) Precipitation Reactions Intended to show precipitate

Slide 7 : 7 Solubility Rules. 1. All compounds containing alkali metal ions and the ammonium ion are soluble. 2. All compounds containing NO3- anions are soluble. 3. All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+ Actually PbCl2 is insoluble in cold but soluble in hot water. 4. All sulphates are soluble except those containing Pb2+, Ca2+ and Ba2+ - actually CaSO4 is sparingly soluble 5. All hydroxides are insoluble except those of the alkali metals, ammonium, Ca2+,  and Ba2+ 6. All carbonates are insoluble except those of the alkali metals and ammonium.

Slide 8 : 8 Some other types of reaction you should know. Acid + Base ? Salt + Water Acid + Metal ? Salt + Hydrogen Acid + Metal ? Salt + CO2 + H2O Carbonate Ammonium + Sodium ? Salt + NH3 + H2O Compound Hydroxide Metal ? Metal + CO2 Carbonate Oxide

1 A part of the Periodic table is shown below.a) Name the Russian scientist whose work led to the development of the modern Periodic Table. ___________________________ [1] : 1 A part of the Periodic table is shown below.a) Name the Russian scientist whose work led to the development of the modern Periodic Table. ___________________________ [1] 2002, Paper 1: Periodic Table, Metals and Non-metals

1 A part of the Periodic table is shown below.a) Name the Russian scientist whose work led to the development of the modern Periodic Table. Mendeleev (similar spelling accepted) [1] : 1 A part of the Periodic table is shown below.a) Name the Russian scientist whose work led to the development of the modern Periodic Table. Mendeleev (similar spelling accepted) [1]

b) Using only the elements shown above name:(i) the most reactive Alkali Metal: ___________________________ [1](ii) the least reactive Halogen: ___________________________ [1] : b) Using only the elements shown above name:(i) the most reactive Alkali Metal: ___________________________ [1](ii) the least reactive Halogen: ___________________________ [1]

b) Using only the elements shown above name: the most reactive Alkali Metal: rubidium the least reactive Halogen: iodine : b) Using only the elements shown above name: the most reactive Alkali Metal: rubidium the least reactive Halogen: iodine

(iii) the least dense Noble Gas: ___________________________ [1](iv) a semi-metal ___________________________ [1] : (iii) the least dense Noble Gas: ___________________________ [1](iv) a semi-metal ___________________________ [1]

(iii) the least dense Noble Gas: helium [1](iv) a semi-metal silicon or germanium [1] : (iii) the least dense Noble Gas: helium [1](iv) a semi-metal silicon or germanium [1]

Slide 15 : 15

Glenn Seaborg(1912-1999) : Glenn Seaborg(1912-1999) Discovered 8 new elements. Only living person for whom an element was named. Seaborgium Sg(106)

(v) a metal of valency 3: ___________________________ [1](vi) two different elements which can exist as allotropes: ___________________________ [1] : (v) a metal of valency 3: ___________________________ [1](vi) two different elements which can exist as allotropes: ___________________________ [1]

(v) a metal of valency 3: aluminium [1](vi) two different elements which can exist as allotropes: carbon [1] and sulphur [1] (Accept oxygen, phosphorus. Accept symbols for all (b)) : (v) a metal of valency 3: aluminium [1](vi) two different elements which can exist as allotropes: carbon [1] and sulphur [1] (Accept oxygen, phosphorus. Accept symbols for all (b))

c) (i) Complete the table below to show the observations which could be made when the two selected elements react under the conditions shown. [13] : c) (i) Complete the table below to show the observations which could be made when the two selected elements react under the conditions shown. [13]

Slide 20 : 20 Magnesium + Steam ? Magnesium Oxide

c) (i) Complete the table below to show the observations which could be made when the two selected elements react under the conditions shown. : c) (i) Complete the table below to show the observations which could be made when the two selected elements react under the conditions shown.

(ii) Write balanced symbol equations for those reactions you think occur. _____________________________ _____________________________ _____________________________ __________________________ [8] : (ii) Write balanced symbol equations for those reactions you think occur. _____________________________ _____________________________ _____________________________ __________________________ [8]

(ii) Write balanced symbol equations for those reactions you think occur. Mg + 2HCl ? MgCl2 + H2 [2] 2Mg + O2 ? 2MgO [2] Mg + H2O ? MgO + H2 [2] S + O2 ? SO2 [2] [1] – Correct symbols used throughout [1] – Correct balancing Accept correct ionic equation : (ii) Write balanced symbol equations for those reactions you think occur. Mg + 2HCl ? MgCl2 + H2 [2] 2Mg + O2 ? 2MgO [2] Mg + H2O ? MgO + H2 [2] S + O2 ? SO2 [2] [1] – Correct symbols used throughout [1] – Correct balancing Accept correct ionic equation

Slide 24 : 24 S + O2 ? SO2

3 From your knowledge of the reactivity series of metals, explain fully the following statements. Give balanced symbol equations where indicated.a) A reaction occurs when copper sulphate is placed in a zinc container. __________________________________ _______________________________ [2] Equation _______________________ [2] : 3 From your knowledge of the reactivity series of metals, explain fully the following statements. Give balanced symbol equations where indicated.a) A reaction occurs when copper sulphate is placed in a zinc container. __________________________________ _______________________________ [2] Equation _______________________ [2] 2002, Paper 2

Slide 26 : 26 Zinc + Copper Sulphate ? Zinc Sulphate + Copper When you have 2 different metals in the same solution you set up an electrochemical cell. This results in other reactions that complicate matters.

Slide 27 : 27

3 From your knowledge of the reactivity series of metals, explain fully the following statements. Give balanced symbol equations where indicated.a) A reaction occurs when copper sulphate is placed in a zinc container. Zinc is higher [1] than copper in the reactivity series and therefore displaces [1] copper. Equation: Zn + CuSO4 ? ZnSO4 + Cu [2] : 3 From your knowledge of the reactivity series of metals, explain fully the following statements. Give balanced symbol equations where indicated.a) A reaction occurs when copper sulphate is placed in a zinc container. Zinc is higher [1] than copper in the reactivity series and therefore displaces [1] copper. Equation: Zn + CuSO4 ? ZnSO4 + Cu [2]

b) Calcium only occurs naturally combined with other elements. __________________________________ _______________________________ [2]c) A mixture of powdered aluminium and iron (III) oxide reacts when heated. _________________________________ _______________________________ [2] Equation _______________________ [2] : b) Calcium only occurs naturally combined with other elements. __________________________________ _______________________________ [2]c) A mixture of powdered aluminium and iron (III) oxide reacts when heated. _________________________________ _______________________________ [2] Equation _______________________ [2]

b) Calcium only occurs naturally combined with other elements. Calcium is a reactive [1] metal and therefore occurs in nature as compounds [1] c) A mixture of powdered aluminium and iron (III) oxide reacts when heated. Aluminium is above [1] iron in the reactivity series and therefore takes the oxygen from iron [1] Equation: 2Al + Fe2O3 ? 2Fe + Al2O3 [2] : b) Calcium only occurs naturally combined with other elements. Calcium is a reactive [1] metal and therefore occurs in nature as compounds [1] c) A mixture of powdered aluminium and iron (III) oxide reacts when heated. Aluminium is above [1] iron in the reactivity series and therefore takes the oxygen from iron [1] Equation: 2Al + Fe2O3 ? 2Fe + Al2O3 [2]

Slide 31 : 31 Thermite demo Thermite welding Underwater welding franklychemistry.com Fe2O3 + 2Al ? 2Fe + Al2O3

d) Potassium metal cannot be extracted by heating the ore with carbon. _____________________________ ___________________________ [2]e) magnesium bars bolted to the hulls of steel ships will prevent rusting. ________________ _____________ [2] : d) Potassium metal cannot be extracted by heating the ore with carbon. _____________________________ ___________________________ [2]e) magnesium bars bolted to the hulls of steel ships will prevent rusting. ________________ _____________ [2]

Slide 33 : 33 Magnesium forms Sacrificial Anodes

Slide 34 : 34 Can you recall the two separate parts to the investigation carried out to determine the factors that control rusting of iron?

Slide 35 : 35 Can you recall the two separate parts to the investigation carried out to determine the factors that control rusting of iron? rust: hydrated [1] iron (III) oxide Formation requires: air [1] and water [1]

Slide 36 : 36 Do you know several methods used to prevent or slow rusting?

Slide 37 : 37 Do you know several methods used to prevent or slow rusting? prevention by: painting [1]; plastic coating [1]; chrome plating [1]; galvanising; [1]; sacrifical protection [1]

d) Potassium metal cannot be extracted by heating the ore with carbon. Potassium is a very reactive [1] metal and can only be extracted by electrolysis [1]e) Magnesium bars bolted to the hulls of steel ships will prevent rusting. Magnesium is more reactive [1] than iron and therefore magnesium will react/first [1]. Accept magnesium is more reactive [1]. It reacts by sacrificial protection [1] : d) Potassium metal cannot be extracted by heating the ore with carbon. Potassium is a very reactive [1] metal and can only be extracted by electrolysis [1]e) Magnesium bars bolted to the hulls of steel ships will prevent rusting. Magnesium is more reactive [1] than iron and therefore magnesium will react/first [1]. Accept magnesium is more reactive [1]. It reacts by sacrificial protection [1]

Slide 39 : 39 Do you know three uses of aluminium and can you explain the properties that make it suitable for these application?

Slide 40 : 40 Do you know three uses of aluminium?

3 Calcium and magnesium are typical alkaline earth metals and they form a variety of compounds. Their compounds show similar chemistry.a) On heating, calcium carbonate decomposed to produce calcium oxide and carbon dioxide. (i) Give two uses of calcium carbonate. ____________________________________ _________________________________ [2] : 3 Calcium and magnesium are typical alkaline earth metals and they form a variety of compounds. Their compounds show similar chemistry.a) On heating, calcium carbonate decomposed to produce calcium oxide and carbon dioxide. (i) Give two uses of calcium carbonate. ____________________________________ _________________________________ [2] 2003, Paper 1

3 Calcium and magnesium are typical alkaline earth metals and they form a variety of compounds. Their compounds show similar chemistry.a) On heating, calcium carbonate decomposed to produce calcium oxide and carbon dioxide. (i) Give two uses of calcium carbonate. Cement manufacture/slag removal in blast furnace/blackboard chalk/reducing acidity in rivers/as a building material/in toothpaste/reducing acidity. Any two [2] : 3 Calcium and magnesium are typical alkaline earth metals and they form a variety of compounds. Their compounds show similar chemistry.a) On heating, calcium carbonate decomposed to produce calcium oxide and carbon dioxide. (i) Give two uses of calcium carbonate. Cement manufacture/slag removal in blast furnace/blackboard chalk/reducing acidity in rivers/as a building material/in toothpaste/reducing acidity. Any two [2]

ii) Draw a labelled diagram of the apparatus used to heat a sample of calcium carbonate safely in a crucible. [3] : ii) Draw a labelled diagram of the apparatus used to heat a sample of calcium carbonate safely in a crucible. [3]

ii) Draw a labelled diagram of the apparatus used to heat a sample of calcium carbonate safely in a crucible.Heat/Bunsen burner [1]Heatproof mat [1]Tripod [1]Gauze/pipeclay triangle [1]Max [3] / [4] : ii) Draw a labelled diagram of the apparatus used to heat a sample of calcium carbonate safely in a crucible.Heat/Bunsen burner [1]Heatproof mat [1]Tripod [1]Gauze/pipeclay triangle [1]Max [3] / [4]

b) Calcium oxide reacts readily with water to form calcium hydroxide solution.(i) What would be observed when water is added dropwise to the calcium oxide produced in part (a)(ii) above? _____________________________ __________________________ [2] : b) Calcium oxide reacts readily with water to form calcium hydroxide solution.(i) What would be observed when water is added dropwise to the calcium oxide produced in part (a)(ii) above? _____________________________ __________________________ [2]

Slide 46 : 46 Steams hisses expands Calcium Oxide + Water JustChemy.Com

b) Calcium oxide reacts readily with water to form calcium hydroxide solution.(i) What would be observed when water is added dropwise to the calcium oxide produced in part (a)(ii) above? Calcium oxide expands [1] heat [1] crumbles [1] hisses water turned into steam Max [2] / [4] : b) Calcium oxide reacts readily with water to form calcium hydroxide solution.(i) What would be observed when water is added dropwise to the calcium oxide produced in part (a)(ii) above? Calcium oxide expands [1] heat [1] crumbles [1] hisses water turned into steam Max [2] / [4]

(ii) Write a balanced, symbol equation for the reaction of calcium oxide with water. ___________________________ [2](iii) What common name is given to calcium hydroxide solution? ___________________________ [1] : (ii) Write a balanced, symbol equation for the reaction of calcium oxide with water. ___________________________ [2](iii) What common name is given to calcium hydroxide solution? ___________________________ [1]

(ii) Write a balanced, symbol equation for the reaction of calcium oxide with water. CaO + H2O ? Ca(OH)2 [2](iii) What common name is given to calcium hydroxide solution? Limewater : (ii) Write a balanced, symbol equation for the reaction of calcium oxide with water. CaO + H2O ? Ca(OH)2 [2](iii) What common name is given to calcium hydroxide solution? Limewater

c) Carbon dioxide gas reacts with calcium hydroxide solution. What would be observed when carbon dioxide is bubbled through calcium hydroxide solution until it is in excess? _____________________________ ___________________________ [3] : c) Carbon dioxide gas reacts with calcium hydroxide solution. What would be observed when carbon dioxide is bubbled through calcium hydroxide solution until it is in excess? _____________________________ ___________________________ [3]

c) Carbon dioxide gas reacts with calcium hydroxide solution. What would be observed when carbon dioxide is bubbled through calcium hydroxide solution until it is in excess? Colourless [1] solution / turns milky [1] / ppt dissolves [1] : c) Carbon dioxide gas reacts with calcium hydroxide solution. What would be observed when carbon dioxide is bubbled through calcium hydroxide solution until it is in excess? Colourless [1] solution / turns milky [1] / ppt dissolves [1]

Slide 52 : 52 From video-tuition. This one is entitled “Limestone Cycle”.

Slide 53 : 53 1. CaCO3 ? CaO + CO2 2. CaO + H2O ? Ca(OH)2 3. Filter & collect filtrate 4. Ca(OH)2 + CO2 ? CaCO3 + H2O 5. CaCO3 + H2O + CO2 ? Ca(HCO3)2 6. Ca(HCO3)2 ? CaCO3 + H2O + CO2

Slide 54 : 54

d) Magnesium metal reacts readily with dilute hydrochloric acid whereas copper metal does not react with the acid.(i) Write a balanced symbol equation for the reaction of magnesium with hydrochloric acid. ______________________________ [2] : d) Magnesium metal reacts readily with dilute hydrochloric acid whereas copper metal does not react with the acid.(i) Write a balanced symbol equation for the reaction of magnesium with hydrochloric acid. ______________________________ [2]

d) Magnesium metal reacts readily with dilute hydrochloric acid whereas copper metal does not react with the acid.(i) Write a balanced symbol equation for the reaction of magnesium with hydrochloric acid. Mg + 2HCl ? MgCl2 + H2 : d) Magnesium metal reacts readily with dilute hydrochloric acid whereas copper metal does not react with the acid.(i) Write a balanced symbol equation for the reaction of magnesium with hydrochloric acid. Mg + 2HCl ? MgCl2 + H2

Give three observations which could be made when magnesium reacts with hydrochloric acid. _______________________________ _______________________________ ____________________________ [3] Explain why magnesium reacts with hydrochloric acid and copper does not. __________________________________ _______________________________ [2] : Give three observations which could be made when magnesium reacts with hydrochloric acid. _______________________________ _______________________________ ____________________________ [3] Explain why magnesium reacts with hydrochloric acid and copper does not. __________________________________ _______________________________ [2] POTASSIUM SODIUM LITHIUM CALCIUM MAGNESIUM ALUMINIUM ZINC IRON LEAD COPPER

(ii) Give three observations which could be made when magnesium reacts with hydrochloric acid. Bubbles/fizzing/gas [1] Temperature increases [1] Magnesium disappears [1] Colourless solution [1] Max [3] / [4] (iii) Explain why magnesium reacts with hydrochloric acid and copper does not. Magnesium is more [1] reactive [1] than copper : (ii) Give three observations which could be made when magnesium reacts with hydrochloric acid. Bubbles/fizzing/gas [1] Temperature increases [1] Magnesium disappears [1] Colourless solution [1] Max [3] / [4] (iii) Explain why magnesium reacts with hydrochloric acid and copper does not. Magnesium is more [1] reactive [1] than copper

(e) Magnesium metal will react with a solution of zinc chloride.(i) Write a balanced ionic equation for this reaction. _____________________________ ___________________________ [2] : (e) Magnesium metal will react with a solution of zinc chloride.(i) Write a balanced ionic equation for this reaction. _____________________________ ___________________________ [2]

(e) Magnesium metal will react with a solution of zinc chloride.(i) Write a balanced ionic equation for this reaction. Mg + Zn2+ ? Mg2+ Zn [2] : (e) Magnesium metal will react with a solution of zinc chloride.(i) Write a balanced ionic equation for this reaction. Mg + Zn2+ ? Mg2+ Zn [2]

(ii) Explain as fully as possible in terms of electrons, why this reaction is described as a redox reaction. Ionic equations may be used to help answer this question. __________________________________ __________________________________ __________________________________ _______________________________ [7] : (ii) Explain as fully as possible in terms of electrons, why this reaction is described as a redox reaction. Ionic equations may be used to help answer this question. __________________________________ __________________________________ __________________________________ _______________________________ [7]

Slide 62 : 62 Oxidation Is Loss Reduction Is Gain

(ii) Explain as fully as possible in terms of electrons, why this reaction is described as a redox reaction. Ionic equations may be used to help answer this question. Magnesium [1] loses electrons [1] (or Mg ? Mg2+ + 2e-[2]) loss of electrons is oxidation [1] accept Mg – 2e- ?Mg2+ Zinc ions [1] gain electrons [1] (or Zn2+ + 2e- ? Zn [2]) gain of electrons is reduction [1] Both oxidation and reduction occurring simultaneously is redox [1] : (ii) Explain as fully as possible in terms of electrons, why this reaction is described as a redox reaction. Ionic equations may be used to help answer this question. Magnesium [1] loses electrons [1] (or Mg ? Mg2+ + 2e-[2]) loss of electrons is oxidation [1] accept Mg – 2e- ?Mg2+ Zinc ions [1] gain electrons [1] (or Zn2+ + 2e- ? Zn [2]) gain of electrons is reduction [1] Both oxidation and reduction occurring simultaneously is redox [1]

2a) A solution of zinc sulphate may be prepared by the addition of an excess of one of the following substances A, B, C or D to dilute sulphuric acid. As well as zinc sulphate solution, each reaction produces at least one other product. : 2a) A solution of zinc sulphate may be prepared by the addition of an excess of one of the following substances A, B, C or D to dilute sulphuric acid. As well as zinc sulphate solution, each reaction produces at least one other product. Hydrogen [1] Water [1] Water [1] Carbon Dioxide [1] Water [1] 2003, Paper 2

(i) Complete boxes 1 to 5 in the diagram to show the names of the other products in the reactions. [5](ii) write balanced, symbol equations for the reaction of dilute sulphuric acid with substances: B _______________________ [2] D _______________________ [2] : (i) Complete boxes 1 to 5 in the diagram to show the names of the other products in the reactions. [5](ii) write balanced, symbol equations for the reaction of dilute sulphuric acid with substances: B _______________________ [2] D _______________________ [2]

(i) Complete boxes 1 to 5 in the diagram to show the names of the other products in the reactions. [5](ii) Write balanced, symbol equations for the reaction of dilute sulphuric acid with substances: B ZnO + H2SO4 ? ZnSO4 + H2O [2] D ZnCO3 + H2SO4 ? ZnSO4 + H2O + CO2 [2] : (i) Complete boxes 1 to 5 in the diagram to show the names of the other products in the reactions. [5](ii) Write balanced, symbol equations for the reaction of dilute sulphuric acid with substances: B ZnO + H2SO4 ? ZnSO4 + H2O [2] D ZnCO3 + H2SO4 ? ZnSO4 + H2O + CO2 [2]

(iii) Give two observations that you would make when the reaction in method D was complete. _____________________________ __________________________ [2] : (iii) Give two observations that you would make when the reaction in method D was complete. _____________________________ __________________________ [2]

(iii) Give two observations that you would make when the reaction in method D was complete. Gas production stops/fizzing stops [1] No more solid reacts/solid remaining [1] : (iii) Give two observations that you would make when the reaction in method D was complete. Gas production stops/fizzing stops [1] No more solid reacts/solid remaining [1]

b) Sulphuric Acid is a strong acid.(i) What is the pH of a sample dilute sulphuric acid? __________________________ [1] : b) Sulphuric Acid is a strong acid.(i) What is the pH of a sample dilute sulphuric acid? __________________________ [1]

b) Sulphuric Acid is a strong acid.(i) What is the pH of a sample dilute sulphuric acid? 0 – 2 [1] : b) Sulphuric Acid is a strong acid.(i) What is the pH of a sample dilute sulphuric acid? 0 – 2 [1]

(ii) Give the name and the formulae of the ions present in all acids and alkalis. : (ii) Give the name and the formulae of the ions present in all acids and alkalis.

(ii) Give the name and the formulae of the ions present in all acids and alkalis. : (ii) Give the name and the formulae of the ions present in all acids and alkalis.

(iii) Write an ionic equation for neutralisation. __________________________ [2] : (iii) Write an ionic equation for neutralisation. __________________________ [2]

(iii) Write an ionic equation for neutralisation. H+ + OH- ? H2O [2] : (iii) Write an ionic equation for neutralisation. H+ + OH- ? H2O [2]

c) It was decided to use substance D to make zinc sulphate by adding an excess of zinc carbonate to sulphuric acid.(i) Explain giving experimental detail, how a pure, dry sample of zinc sulphate, ZnSO4.7H2O, could be prepared from this completed reaction. __________________________________ _______________________________ [6] Quality of written communication [2] : c) It was decided to use substance D to make zinc sulphate by adding an excess of zinc carbonate to sulphuric acid.(i) Explain giving experimental detail, how a pure, dry sample of zinc sulphate, ZnSO4.7H2O, could be prepared from this completed reaction. __________________________________ _______________________________ [6] Quality of written communication [2]

c) It was decided to use substance D to make zinc sulphate by adding an excess of zinc carbonate to sulphuric acid.(i) Explain giving experimental detail, how a pure, dry sample of zinc sulphate, ZnSO4.7H2O, could be prepared from this completed reaction. Filter [1] heat [1] to evaporate some water/to concentrate the solution [1] allow to cool [1] and recrystallise [1] filter [1] dry between two sheets of filter paper / dessicator / low temp oven [1] Quality of written communication [2] : c) It was decided to use substance D to make zinc sulphate by adding an excess of zinc carbonate to sulphuric acid.(i) Explain giving experimental detail, how a pure, dry sample of zinc sulphate, ZnSO4.7H2O, could be prepared from this completed reaction. Filter [1] heat [1] to evaporate some water/to concentrate the solution [1] allow to cool [1] and recrystallise [1] filter [1] dry between two sheets of filter paper / dessicator / low temp oven [1] Quality of written communication [2]

(ii) A sample of zinc sulphate crystals is dissolved in water. Describe how you would test for the presence of the sulphate ion in this solution. Reagent: ______________________ Result: ______________________ ___________________________ [3] : (ii) A sample of zinc sulphate crystals is dissolved in water. Describe how you would test for the presence of the sulphate ion in this solution. Reagent: ______________________ Result: ______________________ ___________________________ [3]

(ii) A sample of zinc sulphate crystals is dissolved in water. Describe how you would test for the presence of the sulphate ion in this solution. Reagent: barium chloride (sodium) [1] Result: white [1] precipitate [1] : (ii) A sample of zinc sulphate crystals is dissolved in water. Describe how you would test for the presence of the sulphate ion in this solution. Reagent: barium chloride (sodium) [1] Result: white [1] precipitate [1]

d) Substance C, zinc hydroxide, was used to prepare zinc sulphate solution.(i) Zinc hydroxide reacts with both acids and alkalis. What term is used to describe this property of zinc hydroxide? ___________________________ [1] : d) Substance C, zinc hydroxide, was used to prepare zinc sulphate solution.(i) Zinc hydroxide reacts with both acids and alkalis. What term is used to describe this property of zinc hydroxide? ___________________________ [1]

d) Substance C, zinc hydroxide, was used to prepare zinc sulphate solution.(i) Zinc hydroxide reacts with both acids and alkalis. What term is used to describe this property of zinc hydroxide? Amphoteric [1] : d) Substance C, zinc hydroxide, was used to prepare zinc sulphate solution.(i) Zinc hydroxide reacts with both acids and alkalis. What term is used to describe this property of zinc hydroxide? Amphoteric [1]

Slide 81 : 81 Zinc and Aluminium metals are Amphoteric. They react with acids and alkalis to form a salt and hydrogen. ACID + Metal ? SALT + Hydrogen Hydrochloric + Zinc ? Zinc + Hydrogen Acid Chloride Hydrochloric + Aluminium ? Aluminium + Hydrogen Acid Chloride

Slide 82 : 82 Zinc and Aluminium metals are Amphoteric. They react with alkalis. Metal + BASE ? SALT + Hydrogen Zinc + Sodium ? Sodium + Hydrogen Hydroxide Zincate Aluminium + Sodium + Water ? Sodium + Hydrogen Hydroxide Aluminate

Slide 83 : 83 Zinc Hydroxide and Aluminium Hydroxide are also Amphoteric. They react with alkalis as follows: - ACID + BASE ? SALT + Water Zinc + Sodium ? Sodium + Water Hydroxide Hydroxide Zincate Zn(OH)2 + 2NaOH ? Na2ZnO2 + 2H2O Aliuminium + Sodium ? Sodium + Water Hydroxide Hydroxide Aluminate Al(OH)3 + NaOH ? NaAlO2 + 2H2O

(ii) Write a balanced, symbol equation for the reaction of zinc hydroxide with sodium hydroxide solution. ___________________________ [3](iii) what other metal hydroxide reacts in a similar way with acids and alkalis? ___________________________ [1] : (ii) Write a balanced, symbol equation for the reaction of zinc hydroxide with sodium hydroxide solution. ___________________________ [3](iii) what other metal hydroxide reacts in a similar way with acids and alkalis? ___________________________ [1]

(ii) Write a balanced, symbol equation for the reaction of zinc hydroxide with sodium hydroxide solution. [3] Zn(OH)2 + 2NaOH ? Na2ZnO2 + 2H2O Allow: Zn(OH)2 + 2NaOH ? Na2Zn(OH)4 And: Zn(OH) 2 + 2OH- ? Zn(OH)42- (iii) what other metal hydroxide reacts in a similar way with acids and alkalis? Aluminium (hydroxide) [1] : (ii) Write a balanced, symbol equation for the reaction of zinc hydroxide with sodium hydroxide solution. [3] Zn(OH)2 + 2NaOH ? Na2ZnO2 + 2H2O Allow: Zn(OH)2 + 2NaOH ? Na2Zn(OH)4 And: Zn(OH) 2 + 2OH- ? Zn(OH)42- (iii) what other metal hydroxide reacts in a similar way with acids and alkalis? Aluminium (hydroxide) [1]

4a) hydrochloric acid reacts with zinc hydroxide and potassium hydroxide. These reactions produce salts. Zinc hydroxide is a base. Potassium hydroxide is an alkali.(i) Name one other base. Any other metal oxide or hydroxide. Not zinc hydroxide / potassium hydroxide. [1](ii) What is meant by the term alkali? Soluble [1] base [1] [2] : 4a) hydrochloric acid reacts with zinc hydroxide and potassium hydroxide. These reactions produce salts. Zinc hydroxide is a base. Potassium hydroxide is an alkali.(i) Name one other base. Any other metal oxide or hydroxide. Not zinc hydroxide / potassium hydroxide. [1](ii) What is meant by the term alkali? Soluble [1] base [1] [2] 2006, Paper 1

b) Zinc hydroxide acts as a base with hydrochloric acid. However, it also reacts with alkalis like potassium hydroxide.(i) What term is used for substances like zinc hydroxide which react with both acids and alkalis? _______________________________ [1](ii) Name one other metal hydroxide which behaves in this way. _______________________________ [1] : b) Zinc hydroxide acts as a base with hydrochloric acid. However, it also reacts with alkalis like potassium hydroxide.(i) What term is used for substances like zinc hydroxide which react with both acids and alkalis? _______________________________ [1](ii) Name one other metal hydroxide which behaves in this way. _______________________________ [1]

b) Zinc hydroxide acts as a base with hydrochloric acid. However, it also reacts with alkalis like potassium hydroxide.(i) What term is used for substances like zinc hydroxide which react with both acids and alkalis? Amphoteric [1](ii) Name one other metal hydroxide which behaves in this way. Aluminium hydroxide [1] : b) Zinc hydroxide acts as a base with hydrochloric acid. However, it also reacts with alkalis like potassium hydroxide.(i) What term is used for substances like zinc hydroxide which react with both acids and alkalis? Amphoteric [1](ii) Name one other metal hydroxide which behaves in this way. Aluminium hydroxide [1]

(iii) Write balanced symbol equations for the reactions between: (1) zinc hydroxide and hydrochloric acid _______________________________ [1] (2) zinc hydroxide and potassium hydroxide _______________________________ [1] : (iii) Write balanced symbol equations for the reactions between: (1) zinc hydroxide and hydrochloric acid _______________________________ [1] (2) zinc hydroxide and potassium hydroxide _______________________________ [1]

(iii) Write balanced symbol equations for the reactions between: (1) zinc hydroxide and hydrochloric acid Zn(OH)2 + 2HCl ? ZnCl2 + 2H2O[1](2) zinc hydroxide and potassium hydroxide Zn(OH)2 + 2KOH ? K2ZnO2 + 2H2O [1] or Zn(OH)2 + 2KOH ? K2Zn(OH)4 [1] : (iii) Write balanced symbol equations for the reactions between: (1) zinc hydroxide and hydrochloric acid Zn(OH)2 + 2HCl ? ZnCl2 + 2H2O[1](2) zinc hydroxide and potassium hydroxide Zn(OH)2 + 2KOH ? K2ZnO2 + 2H2O [1] or Zn(OH)2 + 2KOH ? K2Zn(OH)4 [1]

Slide 91 : c) The reaction between zinc carbonate and hydrochloric acid produces the salt zinc chloride. The diagram below details how pure, dry crystals of zinc chloride may be produced.

(i) What piece of apparatus would you use to measure 23cm3 of hydrochloric acid? _______________________________ [1](ii) Explain why the zinc carbonate is added until it is in excess. _______________________________ _______________________________ [1] : (i) What piece of apparatus would you use to measure 23cm3 of hydrochloric acid? _______________________________ [1](ii) Explain why the zinc carbonate is added until it is in excess. _______________________________ _______________________________ [1]

(i) What piece of apparatus would you use to measure 23cm3 of hydrochloric acid? Measuring cylinder / pipette / burette [1](ii) Explain why the zinc carbonate is added until it is in excess. Ensure all acid reacted [1] : (i) What piece of apparatus would you use to measure 23cm3 of hydrochloric acid? Measuring cylinder / pipette / burette [1](ii) Explain why the zinc carbonate is added until it is in excess. Ensure all acid reacted [1]

(iii) Give one way in which you would know the zinc carbonate is in excess. _______________________________ _______________________________ [1](iv) What is the general name given to the solid trapped by the filter paper? _______________________________ [1] : (iii) Give one way in which you would know the zinc carbonate is in excess. _______________________________ _______________________________ [1](iv) What is the general name given to the solid trapped by the filter paper? _______________________________ [1]

(iii) Give one way in which you would know the zinc carbonate is in excess. Solid remaining / no more gas evolved [1](iv) What is the general name given to the solid trapped by the filter paper? Residue [1] : (iii) Give one way in which you would know the zinc carbonate is in excess. Solid remaining / no more gas evolved [1](iv) What is the general name given to the solid trapped by the filter paper? Residue [1]

(v) What is the general name given to the filtered solution? _______________________________ [1](vi) Explain why crystals form as the solution is cooled. _______________________________ _______________________________ [2] : (v) What is the general name given to the filtered solution? _______________________________ [1](vi) Explain why crystals form as the solution is cooled. _______________________________ _______________________________ [2]

(v) What is the general name given to the filtered solution? Filtrate [1](vi) Explain why crystals form as the solution is cooled. Solubility [1] decreases [1] on cooling or More solute [1] than solution can hold [1] : (v) What is the general name given to the filtered solution? Filtrate [1](vi) Explain why crystals form as the solution is cooled. Solubility [1] decreases [1] on cooling or More solute [1] than solution can hold [1]

(vii) Give two methods of drying the crystals. 1. _____________________________ [1] 2. _____________________________ [1] : (vii) Give two methods of drying the crystals. 1. _____________________________ [1] 2. _____________________________ [1]

(vii) Give two methods of drying the crystals. Between two pieces of filter paper / desiccator / low temperature oven. Any two [2] : (vii) Give two methods of drying the crystals. Between two pieces of filter paper / desiccator / low temperature oven. Any two [2]

d) Zinc chloride consists of zinc ions and chloride ions. The table below describes a chemical test for zinc ions. : d) Zinc chloride consists of zinc ions and chloride ions. The table below describes a chemical test for zinc ions.

d) Zinc chloride consists of zinc ions and chloride ions. The table below describes a chemical test for zinc ions. : d) Zinc chloride consists of zinc ions and chloride ions. The table below describes a chemical test for zinc ions.

(i) Complete the table giving the observations for the test for zinc ions. [2](ii) Write a balanced ionic equation for the reaction between the zinc ions in zinc chloride and hydroxide ions in sodium hydroxide. _______________________________ [3] : (i) Complete the table giving the observations for the test for zinc ions. [2](ii) Write a balanced ionic equation for the reaction between the zinc ions in zinc chloride and hydroxide ions in sodium hydroxide. _______________________________ [3]

(i) Complete the table giving the observations for the test for zinc ions. White [1] precipitate [1] [2](ii) Write a balanced ionic equation for the reaction between the zinc ions in zinc chloride and hydroxide ions in sodium hydroxide. Zn2+ + 2OH- ? Zn(OH)2 [3] [1] [1] + [1] for balancing : (i) Complete the table giving the observations for the test for zinc ions. White [1] precipitate [1] [2](ii) Write a balanced ionic equation for the reaction between the zinc ions in zinc chloride and hydroxide ions in sodium hydroxide. Zn2+ + 2OH- ? Zn(OH)2 [3] [1] [1] + [1] for balancing

3 Sulphur is a non-metallic element found in Group VI. It exists as allotropes.a) Give three physical properties of the element sulphur. _______________________________ _______________________________ _______________________________ [3] : 3 Sulphur is a non-metallic element found in Group VI. It exists as allotropes.a) Give three physical properties of the element sulphur. _______________________________ _______________________________ _______________________________ [3] 2004, Paper 2

3 Sulphur is a non-metallic element found in Group VI. It exists as allotropes. a) Give three physical properties of the element sulphur. Any three of the following: Solid / Yellow/ brittle / does not conduct electricity / does not conduct heat / insoluble in water [3] : 3 Sulphur is a non-metallic element found in Group VI. It exists as allotropes. a) Give three physical properties of the element sulphur. Any three of the following: Solid / Yellow/ brittle / does not conduct electricity / does not conduct heat / insoluble in water [3]

b)(i) Explain what is meant by the term allotrope. _______________________________ _______________________________ [2](ii) Name the three allotropes of sulphur. _______________________________ _______________________________ _______________________________ [3] : b)(i) Explain what is meant by the term allotrope. _______________________________ _______________________________ [2](ii) Name the three allotropes of sulphur. _______________________________ _______________________________ _______________________________ [3]

Slide 107 : 107

b)(i) Explain what is meant by the term allotrope. Different forms of the same element [1] which exist in the same physical state [1](ii) Name the three allotropes of sulphur. Rhombic [1] / Monoclinic [1] / Plastic [1] : b)(i) Explain what is meant by the term allotrope. Different forms of the same element [1] which exist in the same physical state [1](ii) Name the three allotropes of sulphur. Rhombic [1] / Monoclinic [1] / Plastic [1]

c) The following diagram shows the main stages in the manufacture of sulphuric acid from sulphur. : c) The following diagram shows the main stages in the manufacture of sulphuric acid from sulphur.

Slide 110 : 110

(i) What is the name of this process? _______________________________ [1](ii) stage two involves the conversion of sulphur dioxide to sulphur trioxide. Write a balanced symbol equation for this reaction. _______________________________ _______________________________ [3] : (i) What is the name of this process? _______________________________ [1](ii) stage two involves the conversion of sulphur dioxide to sulphur trioxide. Write a balanced symbol equation for this reaction. _______________________________ _______________________________ [3]

(i) What is the name of this process? Contact [1] [1](ii) Stage two involves the conversion of sulphur dioxide to sulphur trioxide. Write a balanced symbol equation for this reaction. 2SO2 + O2 ? 2SO3 [3] : (i) What is the name of this process? Contact [1] [1](ii) Stage two involves the conversion of sulphur dioxide to sulphur trioxide. Write a balanced symbol equation for this reaction. 2SO2 + O2 ? 2SO3 [3]

(iii) Name the catalyst used in the reaction in (c)(ii) above. _______________________________ [1](iv) in stage three, sulphur trioxide is absorbed in concentrated sulphuric acid to produce oleum. Explain why the sulphur trioxide is not normally absorbed directly in water. _______________________________ _______________________________ _______________________________ [2] : (iii) Name the catalyst used in the reaction in (c)(ii) above. _______________________________ [1](iv) in stage three, sulphur trioxide is absorbed in concentrated sulphuric acid to produce oleum. Explain why the sulphur trioxide is not normally absorbed directly in water. _______________________________ _______________________________ _______________________________ [2]

(iii) Name the catalyst used in the reaction in (c)(ii) above. Vanadium(V) oxide/vanadium pentoxide/ V2O5 [1](iv) In stage three, sulphur trioxide is absorbed in concentrated sulphuric acid to produce oleum. Explain why the sulphur trioxide is not normally absorbed directly in water. Forms an unstable/corrosive [1] mist [1] which is difficult to deal with/contain [1] highly exothermic/dangerous [1] (max [2]) : (iii) Name the catalyst used in the reaction in (c)(ii) above. Vanadium(V) oxide/vanadium pentoxide/ V2O5 [1](iv) In stage three, sulphur trioxide is absorbed in concentrated sulphuric acid to produce oleum. Explain why the sulphur trioxide is not normally absorbed directly in water. Forms an unstable/corrosive [1] mist [1] which is difficult to deal with/contain [1] highly exothermic/dangerous [1] (max [2])

d) Explain how dilute sulphuric acid would be prepared safely from concentrated sulphuric acid. _______________________________ _______________________________ _______________________________ [3] : d) Explain how dilute sulphuric acid would be prepared safely from concentrated sulphuric acid. _______________________________ _______________________________ _______________________________ [3]

d) Explain how dilute sulphuric acid would be prepared safely from concentrated sulphuric acid. Always add acid to water [1] slowly [1] with stirring [1] safety glasses [1] (max [3]) : d) Explain how dilute sulphuric acid would be prepared safely from concentrated sulphuric acid. Always add acid to water [1] slowly [1] with stirring [1] safety glasses [1] (max [3])

e) Concentrated sulphuric acid reacts with sugar.(i) What observations would be made during this reaction? _______________________________ _______________________________ [3](ii) Name the products formed. _______________________________ [2] : e) Concentrated sulphuric acid reacts with sugar.(i) What observations would be made during this reaction? _______________________________ _______________________________ [3](ii) Name the products formed. _______________________________ [2]

e) Concentrated sulphuric acid reacts with sugar.(i) What observations would be made during this reaction? black [1] solid/foam [1] swells up and rises [1] warms up/heat [1] bubbles/gas [1] pungent/caramel smell [1] reaction not immediate [1] (max [3]) (ii) Name the products formed. Carbon/charcoal [1] steam/water [1] [2] : e) Concentrated sulphuric acid reacts with sugar.(i) What observations would be made during this reaction? black [1] solid/foam [1] swells up and rises [1] warms up/heat [1] bubbles/gas [1] pungent/caramel smell [1] reaction not immediate [1] (max [3]) (ii) Name the products formed. Carbon/charcoal [1] steam/water [1] [2]

(iii) What property of concentrated sulphuric acid does this reaction illustrate? _______________________________ [1] : (iii) What property of concentrated sulphuric acid does this reaction illustrate? _______________________________ [1]

(iii) What property of concentrated sulphuric acid does this reaction illustrate? Dehydrating [1] : (iii) What property of concentrated sulphuric acid does this reaction illustrate? Dehydrating [1]

f) Concentrated sulphuric acid may be used in the laboratory to produce hydrogen chloride gas.(i) Write a balanced symbol equation for this reaction. _______________________________ [2] : f) Concentrated sulphuric acid may be used in the laboratory to produce hydrogen chloride gas.(i) Write a balanced symbol equation for this reaction. _______________________________ [2]

f) Concentrated sulphuric acid may be used in the laboratory to produce hydrogen chloride gas.(i) Write a balanced symbol equation for this reaction. NaCl + H2SO4 ? NaHSO4 + HCl Na2SO4 equation allowed: 2NaCl + H2SO4 ? Na2So4 + 2HCl [2] : f) Concentrated sulphuric acid may be used in the laboratory to produce hydrogen chloride gas.(i) Write a balanced symbol equation for this reaction. NaCl + H2SO4 ? NaHSO4 + HCl Na2SO4 equation allowed: 2NaCl + H2SO4 ? Na2So4 + 2HCl [2]

(ii) Describe how you would carry out the test for hydrogen chloride gas and state what you would observe. _______________________________ _______________________________ _______________________________ [4] Quality of written communication [2] : (ii) Describe how you would carry out the test for hydrogen chloride gas and state what you would observe. _______________________________ _______________________________ _______________________________ [4] Quality of written communication [2]

(ii) Describe how you would carry out the test for hydrogen chloride gas and state what you would observe. White [1] fumes/smoke [1] glass rod [1] dipped in conc [1] ammonia [1] (max [4]) Quality of written communication [2] : (ii) Describe how you would carry out the test for hydrogen chloride gas and state what you would observe. White [1] fumes/smoke [1] glass rod [1] dipped in conc [1] ammonia [1] (max [4]) Quality of written communication [2] AMMONIUM + ALKALI ? SALT + AMMONIA + WATER COMPD NH4Cl + NaOH ? NaCl + NH3 + H2O

(iii) Write a balanced symbol equation for the reaction in (f)(ii) above. _______________________________ [2] : (iii) Write a balanced symbol equation for the reaction in (f)(ii) above. _______________________________ [2]

(iii) Write a balanced symbol equation for the reaction in (f)(ii) above. NH3 + HCl ? NH4Cl [2] : (iii) Write a balanced symbol equation for the reaction in (f)(ii) above. NH3 + HCl ? NH4Cl [2]

5a) The Periodic Table below shows the elements with atomic numbers 1 to 36. : 5a) The Periodic Table below shows the elements with atomic numbers 1 to 36. 2004, Paper 2

5a) The Periodic Table below shows the elements with atomic numbers 1 to 36. : 5a) The Periodic Table below shows the elements with atomic numbers 1 to 36. Alkali metals [1] Halogens [1]

(i) Name the boxes shown above for groups I and VII giving the name of each group indicated in the Periodic Table. _____________________________ [2] : (i) Name the boxes shown above for groups I and VII giving the name of each group indicated in the Periodic Table. _____________________________ [2]

(i) Name the boxes shown above for groups I and VII giving the name of each group indicated in the Periodic Table. I = Alkali metals VII = Halogens [2] : (i) Name the boxes shown above for groups I and VII giving the name of each group indicated in the Periodic Table. I = Alkali metals VII = Halogens [2]

(ii) Complete the table below using a tick (v) to show whether each group contains reactive or un-reactive elements and whether these elements are metals or non- metals. : (ii) Complete the table below using a tick (v) to show whether each group contains reactive or un-reactive elements and whether these elements are metals or non- metals.

(ii) Complete the table below using a tick (v) to show whether each group contains reactive or un-reactive elements and whether these elements are metals or non- metals. : (ii) Complete the table below using a tick (v) to show whether each group contains reactive or un-reactive elements and whether these elements are metals or non- metals.

b) In the nineteenth century many attempts were made to classify elements and to find a pattern to their properties and reactivity.(i) Which scientist found a repeating pattern of properties for sets of eight elements which he called octaves? _______________________________ [1] : b) In the nineteenth century many attempts were made to classify elements and to find a pattern to their properties and reactivity.(i) Which scientist found a repeating pattern of properties for sets of eight elements which he called octaves? _______________________________ [1]

b) In the nineteenth century many attempts were made to classify elements and to find a pattern to their properties and reactivity.(i) Which scientist found a repeating pattern of properties for sets of eight elements which he called octaves? Newlands [1] : b) In the nineteenth century many attempts were made to classify elements and to find a pattern to their properties and reactivity.(i) Which scientist found a repeating pattern of properties for sets of eight elements which he called octaves? Newlands [1]

Slide 135 : 135 Newlands (1863) arranged the elements in order of increasing atomic mass and noticed that properties appeared to repeat every eighth element. He therefore arranged the 49 elements known at that time into 7 groups. The Noble Gases had yet to be discovered. Newland’s Table worked well up to calcium but then, for example, Iron ended up in the same group with oxygen and sulphur

Slide 136 : 136 I can apply what I have learnt about periodicity to predict the properties of an unfamiliar element(e.g. barium or xenon) Barium will behave like calcium, but it will be more reactive Caesium will be explosive with water since it will be much more reactive than potassium Xenon will be unreactive like all the Noble Gases Astatine will behave like iodine but it will be less reactive.It will be a solid as the m.p. clearly rises as you descend Boron is a metalloid or semi-metal. It will have some metallic and some non-metallic properties Chromium is a transition element. I would expect it to share properties with iron and copper – such as forming ions of different charge and compounds of various colours

(ii) The work of which Russian scientist led to the development of the modern Periodic Table? _______________________________ [1] : (ii) The work of which Russian scientist led to the development of the modern Periodic Table? _______________________________ [1]

(ii) The work of which Russian scientist led to the development of the modern Periodic Table? Mendeleev [1] : (ii) The work of which Russian scientist led to the development of the modern Periodic Table? Mendeleev [1] How modern version differs. 1. Placed in order of Atomic Mass 2. More elements 3. No spaces

Slide 139 : 139 Mendeleev (1869) had a similar idea, but believed that similar properties occurred after periods (horizontal rows) that could vary in length. This allowed elements like iron to be kept away from elements that they did not resemble. He had the foresight to leave spaces for undiscovered elements and he was remarkably accurate in predicting their properties (e.g. silicon)

c) Potassium reacts readily with cold water.(i) What would you observe when potassium reacts with cold water? _______________________________ _______________________________ _______________________________ [4](ii) Write a balanced symbol equation for this reaction. _______________________________ [3] : c) Potassium reacts readily with cold water.(i) What would you observe when potassium reacts with cold water? _______________________________ _______________________________ _______________________________ [4](ii) Write a balanced symbol equation for this reaction. _______________________________ [3]

Slide 141 : 141

c) Potassium reacts readily with cold water.(i) What would you observe when potassium reacts with cold water? Floats on surface/lilac/flame/explosion eventually disappears/moves about surface/fizzing/forms a molten sphere colourless solution remains. Any four. [4](ii) Write a balanced symbol equation for this reaction. 2K + 2H2O ? 2KOH + H2 [3] : c) Potassium reacts readily with cold water.(i) What would you observe when potassium reacts with cold water? Floats on surface/lilac/flame/explosion eventually disappears/moves about surface/fizzing/forms a molten sphere colourless solution remains. Any four. [4](ii) Write a balanced symbol equation for this reaction. 2K + 2H2O ? 2KOH + H2 [3]

Slide 143 : 143 Potassium flame test & Emission spectrum Lilac

Slide 144 : 144 KEY FACTS: ALKALI METALS.High m.p. and b.p. Alkali metals have unusually low m.p. Malleable (can be shaped)Alkali metals are unusually soft. Ductile (can be stretched) Good electrical conductors Good thermal conductors Lustre (shine) Alkali metals tarnish immediately in air. Sonorous (ring when struck)Alkali metals (Li, Na & K) are less dense than water.

d) Answer the following question concerning the three elements listed below.(i) Which one of the three elements is the most reactive? _______________________________ [1] : d) Answer the following question concerning the three elements listed below.(i) Which one of the three elements is the most reactive? _______________________________ [1]

d) Answer the following question concerning the three elements listed below.(i) Which one of the three elements is the most reactive? Sodium [1] : d) Answer the following question concerning the three elements listed below.(i) Which one of the three elements is the most reactive? Sodium [1]

(ii) What would be observed when a piece of freshly cut sodium is exposed to moist air? _______________________________ _______________________________ [2](iii) what would be observed when a piece of magnesium ribbon is heated? _______________________________ _______________________________ _______________________________ [4] : (ii) What would be observed when a piece of freshly cut sodium is exposed to moist air? _______________________________ _______________________________ [2](iii) what would be observed when a piece of magnesium ribbon is heated? _______________________________ _______________________________ _______________________________ [4]

Slide 148 : 148

(ii) What would be observed when a piece of freshly cut sodium is exposed to moist air? Shiny [1] surface becomes tarnished / dull [2](iii) What would be observed when a piece of magnesium ribbon is heated? White [1] light/flame [1] produces heat [1] leaving a white/grey [1] powder/solid [1] Max [4] from [5] : (ii) What would be observed when a piece of freshly cut sodium is exposed to moist air? Shiny [1] surface becomes tarnished / dull [2](iii) What would be observed when a piece of magnesium ribbon is heated? White [1] light/flame [1] produces heat [1] leaving a white/grey [1] powder/solid [1] Max [4] from [5]

5 A student investigated the effect of heat and dilute sulphuric acid on some metal carbonates. The results of the investigation are recorded in the results table below. Some of the results are missing. : 5 A student investigated the effect of heat and dilute sulphuric acid on some metal carbonates. The results of the investigation are recorded in the results table below. Some of the results are missing. 2005 Paper 2

a)(i) What observations are made when copper(II) carbonate is heated? _______________________________ _______________________________ [2](ii) What name is given to this type of reaction? _______________________________ [2] : a)(i) What observations are made when copper(II) carbonate is heated? _______________________________ _______________________________ [2](ii) What name is given to this type of reaction? _______________________________ [2]

a)(i) What observations are made when copper(II) carbonate is heated? Green [1] to black [1] [2](ii) What name is given to this type of reaction? Thermal [1] decomposition [1] [2] : a)(i) What observations are made when copper(II) carbonate is heated? Green [1] to black [1] [2](ii) What name is given to this type of reaction? Thermal [1] decomposition [1] [2]

Slide 153 : 153

(iii) Write a balanced symbol equation for this reaction. _______________________________ [2]b) Hydrated sodium carbonate contains water of crystallisation. Explain what is meant by water of crystallisation. _______________________________ _______________________________ [2] : (iii) Write a balanced symbol equation for this reaction. _______________________________ [2]b) Hydrated sodium carbonate contains water of crystallisation. Explain what is meant by water of crystallisation. _______________________________ _______________________________ [2]

Slide 155 : 155 Soda Crystals are alkaline. The main uses of Soda Crystals are to dissolve grease, soften water, loosen dirt and reduce acidity. Soda Crystals, along with soap and Soap Flakes, were virtually the only domestic cleaners at the turn of the twentieth century. They were used for cleaning and laundry and can even be used in cooking. Still available in free-flowing crystal variety, Soda Crystals are now also available as a liquid version - ideal as a surface cleaner, a trigger spray version and for commercial use in an anti-bacterial formula.   Water of crystallisation refers to water molecules locked up inside the salt crystals. In this case 10 moles of H2O molecules per mole of salt.   Heating washing soda strongly will drive off the water of crystallisation:   Na2CO3.10H2O(s) ? Na2CO3(s) + 10H2O(g)

(iii) Write a balanced symbol equation for this reaction. CuCO3 ? CuO + CO2 [2]b) Hydrated sodium carbonate contains water of crystallisation. Explain what is meant by water of crystallisation. Water chemically combined [1] in the crystal structure [2] : (iii) Write a balanced symbol equation for this reaction. CuCO3 ? CuO + CO2 [2]b) Hydrated sodium carbonate contains water of crystallisation. Explain what is meant by water of crystallisation. Water chemically combined [1] in the crystal structure [2]

c)(i) Name the three products formed when sodium hydrogencarbonate is heated. _________________________ _________________________ _________________________ [3](ii) Why is sodium hydrogencarbonate used in baking bread? _______________________________ _______________________________ [2] : c)(i) Name the three products formed when sodium hydrogencarbonate is heated. _________________________ _________________________ _________________________ [3](ii) Why is sodium hydrogencarbonate used in baking bread? _______________________________ _______________________________ [2]

c)(i) Name the three products formed when sodium hydrogencarbonate is heated. Sodium carbonate [1] carbon dioxide [1] water [1] [3](ii) Why is sodium hydrogencarbonate used in baking bread? CO2 produced [1] bread rises [1] [2] : c)(i) Name the three products formed when sodium hydrogencarbonate is heated. Sodium carbonate [1] carbon dioxide [1] water [1] [3](ii) Why is sodium hydrogencarbonate used in baking bread? CO2 produced [1] bread rises [1] [2]

(iii) Name the colourless solution formed when sodium hydrogencarbonate reacts with dilute sulphuric acid. ______________________________ [1](iv) Write a balanced symbol equation for the reaction of sodium hydrogencarbonate with dilute sulphuric acid. ______________________________ [3] : (iii) Name the colourless solution formed when sodium hydrogencarbonate reacts with dilute sulphuric acid. ______________________________ [1](iv) Write a balanced symbol equation for the reaction of sodium hydrogencarbonate with dilute sulphuric acid. ______________________________ [3]

(iii) Name the colourless solution formed when sodium hydrogencarbonate reacts with dilute sulphuric acid. Sodium sulphate [1](iv) Write a balanced symbol equation for the reaction of sodium hydrogencarbonate with dilute sulphuric acid. 2NaHCO3 + H2SO4 ? Na2SO4 + 2CO2 + 2H2O [3] : (iii) Name the colourless solution formed when sodium hydrogencarbonate reacts with dilute sulphuric acid. Sodium sulphate [1](iv) Write a balanced symbol equation for the reaction of sodium hydrogencarbonate with dilute sulphuric acid. 2NaHCO3 + H2SO4 ? Na2SO4 + 2CO2 + 2H2O [3]

d) A flame test is used to show the presence of certain metal ions in a compound.(i) Describe in detail how a flame test is performed on a sample of a compound. _______________________________ _______________________________ _______________________________ _______________________________ [4] : d) A flame test is used to show the presence of certain metal ions in a compound.(i) Describe in detail how a flame test is performed on a sample of a compound. _______________________________ _______________________________ _______________________________ _______________________________ [4]

d) A flame test is used to show the presence of certain metal ions in a compound.(i) Describe in detail how a flame test is performed on a sample of a compound. Wire [1] Nichrome or flame test rod placed in concentrated hydrochloric acid [1] heated in flame [1] colour [1] observed (Max [4]) or Flame Test Rod [1] moisten in water [1] sample heated in flame [1] colour observed [1] : d) A flame test is used to show the presence of certain metal ions in a compound.(i) Describe in detail how a flame test is performed on a sample of a compound. Wire [1] Nichrome or flame test rod placed in concentrated hydrochloric acid [1] heated in flame [1] colour [1] observed (Max [4]) or Flame Test Rod [1] moisten in water [1] sample heated in flame [1] colour observed [1]

(ii) Complete the following table: : (ii) Complete the following table:

(ii) Complete the following table: : (ii) Complete the following table:

1 Magnesium metal does not occur uncombined in nature. It was first isolated by Sir Humphrey Davy in 1908 by passing an electric current through molten magnesium chloride. Copper metal does occur in nature and has been known for thousands of years. : 1 Magnesium metal does not occur uncombined in nature. It was first isolated by Sir Humphrey Davy in 1908 by passing an electric current through molten magnesium chloride. Copper metal does occur in nature and has been known for thousands of years. 2006, Paper 1

a) Explain why magnesium metal does not occur uncombined in nature but copper metal does. _______________________________ _______________________________ [1] : a) Explain why magnesium metal does not occur uncombined in nature but copper metal does. _______________________________ _______________________________ [1]

a) Explain why magnesium metal does not occur uncombined in nature but copper metal does. Magnesium more reactive [1] than copper [1] (idea of comparison of reactivity) : a) Explain why magnesium metal does not occur uncombined in nature but copper metal does. Magnesium more reactive [1] than copper [1] (idea of comparison of reactivity)

b) Copper and magnesium are typical metals and show similar physical properties. Both conduct electricity and copper’s use in electrical wiring is also due to the fact that it is ductile.(i) What is meant by the term ductile? _______________________________ _______________________________ [1] : b) Copper and magnesium are typical metals and show similar physical properties. Both conduct electricity and copper’s use in electrical wiring is also due to the fact that it is ductile.(i) What is meant by the term ductile? _______________________________ _______________________________ [1]

b) Copper and magnesium are typical metals and show similar physical properties. Both conduct electricity and copper’s use in electrical wiring is also due to the fact that it is ductile.(i) What is meant by the term ductile? Can be drawn out into wires [1] : b) Copper and magnesium are typical metals and show similar physical properties. Both conduct electricity and copper’s use in electrical wiring is also due to the fact that it is ductile.(i) What is meant by the term ductile? Can be drawn out into wires [1]

(ii) Explain why metals conduct electricity. _______________________________ _______________________________ _______________________________ [3](iii) Give two other physical properties of metals. 1. _____________________________ [1] 2. _____________________________ [1] : (ii) Explain why metals conduct electricity. _______________________________ _______________________________ _______________________________ [3](iii) Give two other physical properties of metals. 1. _____________________________ [1] 2. _____________________________ [1]

Slide 171 : 171 Ca+ion

(ii) Explain why metals conduct electricity. Moving [1] (sea of) electrons [1] (which) carry charge [1] [3] (iii) Give two other physical properties of metals. Malleable, sonorous, lustrous, conducts heat, high melting point, dense/high density, strong. Do not accept: hard, solid, insoluble in water, flexible. Any two [2] : (ii) Explain why metals conduct electricity. Moving [1] (sea of) electrons [1] (which) carry charge [1] [3] (iii) Give two other physical properties of metals. Malleable, sonorous, lustrous, conducts heat, high melting point, dense/high density, strong. Do not accept: hard, solid, insoluble in water, flexible. Any two [2]

c) Compounds of copper vary in their colour. Complete the table below, giving the colour of the substances listed. : c) Compounds of copper vary in their colour. Complete the table below, giving the colour of the substances listed.

Slide 174 : 174 Copper (II) Chloride Copper (II) Hydroxide Green Light Blue

c) Compounds of copper vary in their colour. Complete the table below, giving the colour of the substances listed. : c) Compounds of copper vary in their colour. Complete the table below, giving the colour of the substances listed.

d) Magnesium metal burns in air with a bright white flame as shown below. The product of the reaction is mainly magnesium oxide with about 10% magnesium nitride. : d) Magnesium metal burns in air with a bright white flame as shown below. The product of the reaction is mainly magnesium oxide with about 10% magnesium nitride.

(i) Describe the appearance of magnesium oxide. _______________________________ [2](ii) Write a balanced symbol equation for the formation of the magnesium oxide. _______________________________ [3] : (i) Describe the appearance of magnesium oxide. _______________________________ [2](ii) Write a balanced symbol equation for the formation of the magnesium oxide. _______________________________ [3]

(i) Describe the appearance of magnesium oxide. White [1] solid/powder/dust/ash [2](ii) Write a balanced symbol equation for the formation of the magnesium oxide. 2Mg + O2 ? 2MgO [1] [1] + [1] for balancing [3] : (i) Describe the appearance of magnesium oxide. White [1] solid/powder/dust/ash [2](ii) Write a balanced symbol equation for the formation of the magnesium oxide. 2Mg + O2 ? 2MgO [1] [1] + [1] for balancing [3]

(iii) Give the formula of magnesium nitride. _______________________________ [1]e) Magnesium metal reacts with dilute hydrochloric acid.(i) What would you observe when magnesium reacts with dilute hydrochloric acid? _______________________________ [2] : (iii) Give the formula of magnesium nitride. _______________________________ [1]e) Magnesium metal reacts with dilute hydrochloric acid.(i) What would you observe when magnesium reacts with dilute hydrochloric acid? _______________________________ [2]

Slide 180 : 180 Mg Al Zn Fe Pb Cu

(iii) Give the formula of magnesium nitride. Mg3N2 [1]e) Magnesium metal reacts with dilute hydrochloric acid.(i) What would you observe when magnesium reacts with dilute hydrochloric acid? Heat evolved/temp increases [1] bubbles / idea of [1] Mg disappears [1] (not dissolves) colourless solution [1]. Any two [2] : (iii) Give the formula of magnesium nitride. Mg3N2 [1]e) Magnesium metal reacts with dilute hydrochloric acid.(i) What would you observe when magnesium reacts with dilute hydrochloric acid? Heat evolved/temp increases [1] bubbles / idea of [1] Mg disappears [1] (not dissolves) colourless solution [1]. Any two [2]

(ii) Write a balanced symbol equation for the reaction between magnesium and dilute hydrochloric acid. _______________________________ [3](iii) Name one other metal which reacts safely with dilute hydrochloric. _______________________________ [1] : (ii) Write a balanced symbol equation for the reaction between magnesium and dilute hydrochloric acid. _______________________________ [3](iii) Name one other metal which reacts safely with dilute hydrochloric. _______________________________ [1]

(ii) Write a balanced symbol equation for the reaction between magnesium and dilute hydrochloric acid. Mg + 2HCl ? MgCl2 + H2 [3] [1] [1] + [1] for balancing(iii) Name one other metal which reacts safely with dilute hydrochloric. Calcium / aluminium / zinc / iron [1] : (ii) Write a balanced symbol equation for the reaction between magnesium and dilute hydrochloric acid. Mg + 2HCl ? MgCl2 + H2 [3] [1] [1] + [1] for balancing(iii) Name one other metal which reacts safely with dilute hydrochloric. Calcium / aluminium / zinc / iron [1]

3 The diagram below shows a blast furnace for the production of iron. : 3 The diagram below shows a blast furnace for the production of iron. 2006, Paper 2

Slide 185 : 185 Hot waste gases used to warm incoming air 1800 4000C Called a “charge” Steel reinforced with fire brick “casting”

Slide 186 : 186 Haematite Fe2O3 Magnetite Fe3O4 Fe3O4 is a “compound oxide”: FeO and Fe2O3

Slide 187 : 187 Limestone CaCO3 Limestone CaCO3 CaCO3 ? CaO + CO2 Heat strongly Limestone , indirectly, removes the acidic impurity called silica SiO2

Slide 188 : 188 Extraction of Iron   Extraction of Iron – carried out in the blast furnace [1]   Charge: iron ore [1]; limestone [1]; coke [1]   Hot [1] air [1] blasted in through pipes at bottom of furnace   Reducing agent: carbon monoxide [1]   Reduction of iron ore as oxygen [1] is removed [1] from the iron (III) oxide or Fe3+ ions [1] gain electrons [1] to form Fe [1]

Slide 189 : 189 Stage 1 coke burns in oxygen to produce carbon dioxide [1] C + O2 ? CO2 [2]   Stage 2 carbon dioxide reacts with more coke to produce carbon monoxide [1] CO2 + C ? 2CO [3]   Stage 3 iron (III) oxide reacts with carbon monoxide to produce molten iron [1] and carbon dioxide Fe2O3 + 3CO ? 2Fe + 3CO2 [3] Stage 4 calcium carbonate thermally decomposes to form calcium oxide and carbon dioxide [1] CaCO3 ? CaO + CO2 [2]   Stage 5 silicon dioxide impurities react with calcium oxide to remove impurities as molten slag (= calcium silicate, CaSiO3) SiO2 + CaO ? CaSiO3 [2]

a)(i) Complete the table to give information about the main raw materials which are fed into the top of the blast furnace. [6] : a)(i) Complete the table to give information about the main raw materials which are fed into the top of the blast furnace. [6]

a)(i) Complete the table to give information about the main raw materials which are fed into the top of the blast furnace. [6] : a)(i) Complete the table to give information about the main raw materials which are fed into the top of the blast furnace. [6]

(ii) Name the raw material which is blasted into the furnace at point A. _______________________________ [1](iii) Name the substances tapped off at points B and C. B _____________________________ [1] C _____________________________ [1] : (ii) Name the raw material which is blasted into the furnace at point A. _______________________________ [1](iii) Name the substances tapped off at points B and C. B _____________________________ [1] C _____________________________ [1]

(ii) Name the raw material which is blasted into the furnace at point A. (hot) air [1](iii) Name the substances tapped off at points B and C. B (molten) slag [1] C (molten) iron [1] : (ii) Name the raw material which is blasted into the furnace at point A. (hot) air [1](iii) Name the substances tapped off at points B and C. B (molten) slag [1] C (molten) iron [1]

Slide 194 : 194 Uses of Iron

Slide 195 : 195 SLAG Rail ballast

b) At what bottom of the blast furnace, coke reacts to form carbon dioxide. Write a balanced symbol equation for this reaction. _______________________________ [2]c) The carbon dioxide reacts with more coke to form carbon monoxide.(i) Write a balanced symbol equation for this reaction. _______________________________ [3] : b) At what bottom of the blast furnace, coke reacts to form carbon dioxide. Write a balanced symbol equation for this reaction. _______________________________ [2]c) The carbon dioxide reacts with more coke to form carbon monoxide.(i) Write a balanced symbol equation for this reaction. _______________________________ [3]

b) At what bottom of the blast furnace, coke reacts to form carbon dioxide. Write a balanced symbol equation for this reaction. C + O2 ? CO2 [2]c) The carbon dioxide reacts with more coke to form carbon monoxide.(i) Write a balanced symbol equation for this reaction. CO2 + C ? 2CO [3] [1] [1] +[1] for balancing : b) At what bottom of the blast furnace, coke reacts to form carbon dioxide. Write a balanced symbol equation for this reaction. C + O2 ? CO2 [2]c) The carbon dioxide reacts with more coke to form carbon monoxide.(i) Write a balanced symbol equation for this reaction. CO2 + C ? 2CO [3] [1] [1] +[1] for balancing

(ii) What is the importance of carbon monoxide in the extraction process? _______________________________ [1](iii) Write a balanced symbol equation to show the part played by the carbon monoxide in the extraction process. _______________________________ [3] : (ii) What is the importance of carbon monoxide in the extraction process? _______________________________ [1](iii) Write a balanced symbol equation to show the part played by the carbon monoxide in the extraction process. _______________________________ [3]

(ii) What is the importance of carbon monoxide in the extraction process? Reducing agent/removes oxygen from haematite [1](iii) Write a balanced symbol equation to show the part played by the carbon monoxide in the extraction process. 3CO + Fe2O3 ? 2CO2 + 2Fe [3] [1] [1] +[1] for balancing : (ii) What is the importance of carbon monoxide in the extraction process? Reducing agent/removes oxygen from haematite [1](iii) Write a balanced symbol equation to show the part played by the carbon monoxide in the extraction process. 3CO + Fe2O3 ? 2CO2 + 2Fe [3] [1] [1] +[1] for balancing

d) Sand (SiO2) is an impurity in the raw materials. The sand is removed from the blast furnace by reacting it with calcium oxide.(i) Write a balanced symbol equation for the reaction of sand with calcium oxide. _______________________________ [2] : d) Sand (SiO2) is an impurity in the raw materials. The sand is removed from the blast furnace by reacting it with calcium oxide.(i) Write a balanced symbol equation for the reaction of sand with calcium oxide. _______________________________ [2]

d) Sand (SiO2) is an impurity in the raw materials. The sand is removed from the blast furnace by reacting it with calcium oxide.(i) Write a balanced symbol equation for the reaction of sand with calcium oxide. CaCO3 ? CaO + CO2 [2] [1] [1] : d) Sand (SiO2) is an impurity in the raw materials. The sand is removed from the blast furnace by reacting it with calcium oxide.(i) Write a balanced symbol equation for the reaction of sand with calcium oxide. CaCO3 ? CaO + CO2 [2] [1] [1]

(ii) Write a balanced symbol equation for the reaction of sand with calcium oxide. _______________________________ [2] : (ii) Write a balanced symbol equation for the reaction of sand with calcium oxide. _______________________________ [2]

(ii) Write a balanced symbol equation for the reaction of sand with calcium oxide. CaO + SiO2 ? CaSiO3 [2] [1] [1] : (ii) Write a balanced symbol equation for the reaction of sand with calcium oxide. CaO + SiO2 ? CaSiO3 [2] [1] [1]

e) Large quantities of limestone for use in the blast furnace are obtained from quarries. Give two environmental problems that could be caused by quarrying limestone. _______________________________ _______________________________ [2] : e) Large quantities of limestone for use in the blast furnace are obtained from quarries. Give two environmental problems that could be caused by quarrying limestone. _______________________________ _______________________________ [2]

Slide 205 : 205 Limestone Quarry

Slide 206 : 206 Noisy, dusty and an eyesore

e) Large quantities of limestone for use in the blast furnace are obtained from quarries. Give two environmental problems that could be caused by quarrying limestone. Eyesore [1] loss of animal habitat [1] noise pollution [1] dust pollution [1] damage to landscape [1] traffic density [1] limestone resources depleted [1]. Maximum [2] : e) Large quantities of limestone for use in the blast furnace are obtained from quarries. Give two environmental problems that could be caused by quarrying limestone. Eyesore [1] loss of animal habitat [1] noise pollution [1] dust pollution [1] damage to landscape [1] traffic density [1] limestone resources depleted [1]. Maximum [2]

3 Many calcium containing compounds such as limestone (calcium carbonate) and gypsum (hydrated calcium sulphate) occur naturally.a) Plaster of Paris is formed by heating gypsum to just above 100°C: CaSO4.2H2O ? CaSO4.½H2O + 1½H2O gypsum Plaster of Paris : 3 Many calcium containing compounds such as limestone (calcium carbonate) and gypsum (hydrated calcium sulphate) occur naturally.a) Plaster of Paris is formed by heating gypsum to just above 100°C: CaSO4.2H2O ? CaSO4.½H2O + 1½H2O gypsum Plaster of Paris 2007, Paper 1

Slide 209 : 209 Plaster of Paris Plaster Cast Plaster Mouding CaSO4.½H2O

(i) Calculate the percentage of water present in gypsum _______________________________ _______________________________ _______________________________ [3] : (i) Calculate the percentage of water present in gypsum _______________________________ _______________________________ _______________________________ [3]

(i) Calculate the percentage of water present in gypsum RFM gypsum = (40 + 32 + 4 x 16 + 2 x 8 = 136 + 36=) 172 [1] % H2O = [1] x 100 = 20.9% [1] apply consequential marking [3] : (i) Calculate the percentage of water present in gypsum RFM gypsum = (40 + 32 + 4 x 16 + 2 x 8 = 136 + 36=) 172 [1] % H2O = [1] x 100 = 20.9% [1] apply consequential marking [3]

(ii) State one other use of calcium sulphate _______________________________ [1](iii) What is meant by the term hydrated? _______________________________ [1] : (ii) State one other use of calcium sulphate _______________________________ [1](iii) What is meant by the term hydrated? _______________________________ [1]

(ii) State one other use of calcium sulphate Blackboard chalk / white line road markings / plaster (board) cement [1](iii) What is meant by the term hydrated? Contains water (of crystallisation) [1] : (ii) State one other use of calcium sulphate Blackboard chalk / white line road markings / plaster (board) cement [1](iii) What is meant by the term hydrated? Contains water (of crystallisation) [1]

b) In industry, limestone undergoes thermal decomposition to make quicklime (calcium oxide). The diagram below represents a limekiln which is used for this process. : b) In industry, limestone undergoes thermal decomposition to make quicklime (calcium oxide). The diagram below represents a limekiln which is used for this process.

Slide 215 : 215 Old Limestone Kiln

(i) What is meant by the term thermal decomposition? _______________________________ _______________________________ [2](ii) Write a balanced symbol equation for the thermal decomposition of limestone. _______________________________ [2] : (i) What is meant by the term thermal decomposition? _______________________________ _______________________________ [2](ii) Write a balanced symbol equation for the thermal decomposition of limestone. _______________________________ [2]

(i) What is meant by the term thermal decomposition? Break up [1], using heat [1] [2](ii) Write a balanced symbol equation for the thermal decomposition of limestone. CaCO3 ? CaO + CO2 [2] : (i) What is meant by the term thermal decomposition? Break up [1], using heat [1] [2](ii) Write a balanced symbol equation for the thermal decomposition of limestone. CaCO3 ? CaO + CO2 [2]

(iii) The decomposition of limestone is endothermic. What is the meaning of the term endothermic? _______________________________ _______________________________ [2](iv) Name the main element present in coke. _______________________________ [1] : (iii) The decomposition of limestone is endothermic. What is the meaning of the term endothermic? _______________________________ _______________________________ [2](iv) Name the main element present in coke. _______________________________ [1]

(iii) The decomposition of limestone is endothermic. What is the meaning of the term endothermic? Heat/energy [1] taken in [1] [2](iv) Name the main element present in coke. Carbon [1] : (iii) The decomposition of limestone is endothermic. What is the meaning of the term endothermic? Heat/energy [1] taken in [1] [2](iv) Name the main element present in coke. Carbon [1]

(v) Explain why air is blown into the kiln. _______________________________ _______________________________ [1](vi) Name the gas A which escapes from the top of the kiln. _______________________________ [1] : (v) Explain why air is blown into the kiln. _______________________________ _______________________________ [1](vi) Name the gas A which escapes from the top of the kiln. _______________________________ [1]

(v) Explain why air is blown into the kiln. to allow the coke to burn [1](vi) Name the gas A which escapes from the top of the kiln. Carbon dioxide [1] : (v) Explain why air is blown into the kiln. to allow the coke to burn [1](vi) Name the gas A which escapes from the top of the kiln. Carbon dioxide [1]

(vii) State one other use of calcium carbonate. _______________________________ [1] : (vii) State one other use of calcium carbonate. _______________________________ [1]

(vii) State one other use of calcium carbonate. cement manufacture / blackboard chalk / slag removal from blast furnace / sculptures / statues / fireplaces / neutralise lakes / neutralised acidic soils / in agriculture [1] : (vii) State one other use of calcium carbonate. cement manufacture / blackboard chalk / slag removal from blast furnace / sculptures / statues / fireplaces / neutralise lakes / neutralised acidic soils / in agriculture [1]

Slide 224 : 224 Lime used to neutralise acid

Slide 225 : 225 Manufacture of Cement

Slide 226 : 226 Quicklime (CaO) is used to: 1. Treat acidic impurities in the Blast Furnace. Limestone breaks down to form quicklime: CaCO3 ? CaO + CO2 Acidic silica (SiO2) then reacts with the quicklime to form slag SiO2 + CaO ? CaSiO3 2. Raise the temperature and pH of sewage, helping to kill bacteria. 3. Produce slaked lime. CaO + H2O ? Ca(OH)2

c) In the laboratory, calcium carbonate reacts with hydrochloric acid to produce calcium chloride solution.(i) Write a balanced symbol equation for this reaction. _______________________________ [1] : c) In the laboratory, calcium carbonate reacts with hydrochloric acid to produce calcium chloride solution.(i) Write a balanced symbol equation for this reaction. _______________________________ [1]

c) In the laboratory, calcium carbonate reacts with hydrochloric acid to produce calcium chloride solution.(i) Write a balanced symbol equation for this reaction. CaCO3 + 2HCl ? CaCl2 + CO2 + H2O [1] : c) In the laboratory, calcium carbonate reacts with hydrochloric acid to produce calcium chloride solution.(i) Write a balanced symbol equation for this reaction. CaCO3 + 2HCl ? CaCl2 + CO2 + H2O [1]

(ii) State two observations you would make during this reaction. _______________________________ _______________________________ [2](iii) Sodium hydroxide solution is added slowly to the solution of calcium chloride. What would you observe? _______________________________ _______________________________ [1] : (ii) State two observations you would make during this reaction. _______________________________ _______________________________ [2](iii) Sodium hydroxide solution is added slowly to the solution of calcium chloride. What would you observe? _______________________________ _______________________________ [1]

(ii) State two observations you would make during this reaction. Effervescence / gas produced / bubbles [1] calcium carbonate disappears [1] heat [1] colourless [1] solution. Max [2] (iii) Sodium hydroxide solution is added slowly to the solution of calcium chloride. What would you observe? White [1] ppt/solid [1] [2] : (ii) State two observations you would make during this reaction. Effervescence / gas produced / bubbles [1] calcium carbonate disappears [1] heat [1] colourless [1] solution. Max [2] (iii) Sodium hydroxide solution is added slowly to the solution of calcium chloride. What would you observe? White [1] ppt/solid [1] [2]

(iv) A flame test is carried out using the solution of calcium chloride. State the flame colour observed. _______________________________ [1] : (iv) A flame test is carried out using the solution of calcium chloride. State the flame colour observed. _______________________________ [1]

Slide 232 : 232 Calcium Brick Red

(iv) A flame test is carried out using the solution of calcium chloride. State the flame colour observed. Red/brick-red [1] : (iv) A flame test is carried out using the solution of calcium chloride. State the flame colour observed. Red/brick-red [1]

Slide 234 : 234

Slide 235 : 235

Slide 236 : 236

1a) To investigate the conditions necessary for rusting to occur, the following experiment was carried out. After one week only one of the nails showed signs of rust. : 1a) To investigate the conditions necessary for rusting to occur, the following experiment was carried out. After one week only one of the nails showed signs of rust. 2004, Paper 1

(i) Why was the water in tube C boiled? __________________________ [1](ii) What is the purpose of the olive oil layer in tube C? __________________________ [1] : (i) Why was the water in tube C boiled? __________________________ [1](ii) What is the purpose of the olive oil layer in tube C? __________________________ [1]

(i) Why was the water in tube C boiled? To remove air (allow to remove oxygen [1](ii) What is the purpose of the olive oil layer in tube C? To prevent oxygen/air entering [1] : (i) Why was the water in tube C boiled? To remove air (allow to remove oxygen [1](ii) What is the purpose of the olive oil layer in tube C? To prevent oxygen/air entering [1]

(iii) What is the purpose of the anhydrous calcium chloride? __________________________ [1](iv) Name a substance that could be used instead of anhydrous calcium. __________________________ [1] : (iii) What is the purpose of the anhydrous calcium chloride? __________________________ [1](iv) Name a substance that could be used instead of anhydrous calcium. __________________________ [1]

(iii) What is the purpose of the anhydrous calcium chloride? To remove water/moisture/act as a drying agent [1](iv) Name a substance that could be used instead of anhydrous calcium. Silica gel [1] : (iii) What is the purpose of the anhydrous calcium chloride? To remove water/moisture/act as a drying agent [1](iv) Name a substance that could be used instead of anhydrous calcium. Silica gel [1]

(v) In which test tube will the nail have rusted? __________________________ [1](vi) from the results of this experiment, state the conditions necessary for rusting of iron to occur. __________________________ [1] : (v) In which test tube will the nail have rusted? __________________________ [1](vi) from the results of this experiment, state the conditions necessary for rusting of iron to occur. __________________________ [1]

(v) In which test tube will the nail have rusted? Tube A [1](vi) From the results of this experiment, state the conditions necessary for rusting of iron to occur. Air/oxygen [1] Water/moisture [1] : (v) In which test tube will the nail have rusted? Tube A [1](vi) From the results of this experiment, state the conditions necessary for rusting of iron to occur. Air/oxygen [1] Water/moisture [1]

(vii) What is the full chemical name for rust? __________________________ [1] : (vii) What is the full chemical name for rust? __________________________ [1]

(vii) What is the full chemical name for rust? Hydrated [1] iron(III) oxide [1] : (vii) What is the full chemical name for rust? Hydrated [1] iron(III) oxide [1]

b) Iron can be protected from rusting by sacrificial protection. The diagram below shows an experiment which can be used to investigate the process of sacrificial protection. Different metals are wrapped around iron nails and left in water for one week. : b) Iron can be protected from rusting by sacrificial protection. The diagram below shows an experiment which can be used to investigate the process of sacrificial protection. Different metals are wrapped around iron nails and left in water for one week.

(i) Give two ways in which you could ensure that this experiment was a fair test. ______________________________ ___________________________ [2] : (i) Give two ways in which you could ensure that this experiment was a fair test. ______________________________ ___________________________ [2]

(i) Give two ways in which you could ensure that this experiment was a fair test. Same volume of water [1] same mass of metal [1] same type/size of nail [1] kept in same temperature [1]. Any two : (i) Give two ways in which you could ensure that this experiment was a fair test. Same volume of water [1] same mass of metal [1] same type/size of nail [1] kept in same temperature [1]. Any two

(ii) Explain what is meant by the phrase “sacrificial protection” ______________________________ ___________________________ [2](iii) At the end of the week in which tube(s) would rusting have occurred? ___________________________ [1] : (ii) Explain what is meant by the phrase “sacrificial protection” ______________________________ ___________________________ [2](iii) At the end of the week in which tube(s) would rusting have occurred? ___________________________ [1]

(ii) Explain what is meant by the phrase “sacrificial protection” a metal more reactive [1] than iron reacts/corrodes instead of/before/in preference to (the iron) [2] (iii) At the end of the week in which tube(s) would rusting have occurred? Tube A/tube with copper in it [1] : (ii) Explain what is meant by the phrase “sacrificial protection” a metal more reactive [1] than iron reacts/corrodes instead of/before/in preference to (the iron) [2] (iii) At the end of the week in which tube(s) would rusting have occurred? Tube A/tube with copper in it [1]

(iv) In industry iron is often covered with zinc. What is the name for this process? ___________________________ [1] : (iv) In industry iron is often covered with zinc. What is the name for this process? ___________________________ [1]

(iv) In industry iron is often covered with zinc. What is the name for this process? Galvanising [1] : (iv) In industry iron is often covered with zinc. What is the name for this process? Galvanising [1]

c) Iron filings are used to coat fireworks called sparklers. When the firework is lit the iron burns to produce iron oxide Fe3O4. the sparkler will burn much better in pure oxygen than in air. : c) Iron filings are used to coat fireworks called sparklers. When the firework is lit the iron burns to produce iron oxide Fe3O4. the sparkler will burn much better in pure oxygen than in air.

(i) Write a balanced symbol equation for the reaction that occurs when the iron in the sparkler burns. ___________________________ [2] : (i) Write a balanced symbol equation for the reaction that occurs when the iron in the sparkler burns. ___________________________ [2]

(i) Write a balanced symbol equation for the reaction that occurs when the iron in the sparkler burns. 3Fe + 2O2 ? Fe3O4 [2] : (i) Write a balanced symbol equation for the reaction that occurs when the iron in the sparkler burns. 3Fe + 2O2 ? Fe3O4 [2]

(ii) When the sparkler burns an oxidation reaction occurs. Complete the table, using all the words addition and removal to give the common definitions of oxidation and reduction. : (ii) When the sparkler burns an oxidation reaction occurs. Complete the table, using all the words addition and removal to give the common definitions of oxidation and reduction.

(ii) When the sparkler burns an oxidation reaction occurs. Complete the table, using all the words addition and removal to give the common definitions of oxidation and reduction. : (ii) When the sparkler burns an oxidation reaction occurs. Complete the table, using all the words addition and removal to give the common definitions of oxidation and reduction.

(iii) State the underlined substance is oxidised or reduced in the following reactions: Rusting of iron _________________ Reaction of iron oxide with hydrogen ___________________ [2] : (iii) State the underlined substance is oxidised or reduced in the following reactions: Rusting of iron _________________ Reaction of iron oxide with hydrogen ___________________ [2]

(iii) State the underlined substance is oxidised or reduced in the following reactions: Rusting of iron oxidised [1] Reaction of iron oxide with hydrogen reduced [1] : (iii) State the underlined substance is oxidised or reduced in the following reactions: Rusting of iron oxidised [1] Reaction of iron oxide with hydrogen reduced [1]

4a) Zinc is used in the manufacture of coins. The two pound coin shown below contains a mixture of metals. It is 70% copper, 24.4% zinc and 5.5% nickel. : 4a) Zinc is used in the manufacture of coins. The two pound coin shown below contains a mixture of metals. It is 70% copper, 24.4% zinc and 5.5% nickel. 2004, Paper 1

(i) What is the word used for a substance made up of a mixture of metals? _________________________ [1](ii) Copper, zinc and nickel are malleable. What is meant by the word malleable? ______________________________ _________________________ [1] : (i) What is the word used for a substance made up of a mixture of metals? _________________________ [1](ii) Copper, zinc and nickel are malleable. What is meant by the word malleable? ______________________________ _________________________ [1]

(i) What is the word used for a substance made up of a mixture of metals? Alloy [1](ii) Copper, zinc and nickel are malleable. What is meant by the word malleable? Hammered into shape [1] : (i) What is the word used for a substance made up of a mixture of metals? Alloy [1](ii) Copper, zinc and nickel are malleable. What is meant by the word malleable? Hammered into shape [1]

b) To find out the order of reactivity of copper, nickel and zinc, an excess of each metal was placed into the same concentration of different metal salt solutions. The table below illustrates the results. v = reaction occurred x = no reaction : b) To find out the order of reactivity of copper, nickel and zinc, an excess of each metal was placed into the same concentration of different metal salt solutions. The table below illustrates the results. v = reaction occurred x = no reaction

Write down the order of reactivity of these three metals from most to least reactive. Most reactive = ________________ ________________ Least reactive = ________________ : Write down the order of reactivity of these three metals from most to least reactive. Most reactive = ________________ ________________ Least reactive = ________________

Write down the order of reactivity of these three metals from most to least reactive. Most reactive = Zinc Nickle Opposite order [1] Least reactive = Copper : Write down the order of reactivity of these three metals from most to least reactive. Most reactive = Zinc Nickle Opposite order [1] Least reactive = Copper

c) Zinc reacts with copper(II) sulphate solution producing zinc sulphate and copper.(i) Describe what would be observed in the reaction between zinc metal and copper(II) sulphate solution. ______________________________ ___________________________ [3] : c) Zinc reacts with copper(II) sulphate solution producing zinc sulphate and copper.(i) Describe what would be observed in the reaction between zinc metal and copper(II) sulphate solution. ______________________________ ___________________________ [3]

c) Zinc reacts with copper(II) sulphate solution producing zinc sulphate and copper.(i) Describe what would be observed in the reaction between zinc metal and copper(II) sulphate solution. Brown/red [1] grey metal [1] zinc disappears [1] coating/solid [1] blue colour [1] warms up heat [1] fades/green/colourless solution [1] (max [3] from [7]) : c) Zinc reacts with copper(II) sulphate solution producing zinc sulphate and copper.(i) Describe what would be observed in the reaction between zinc metal and copper(II) sulphate solution. Brown/red [1] grey metal [1] zinc disappears [1] coating/solid [1] blue colour [1] warms up heat [1] fades/green/colourless solution [1] (max [3] from [7])

(ii) The reaction in (c)(i) is a redox reaction. Explain in terms of electrons what this means as applied to this reaction. (You may use ionic equations to help answer this question). ______________________________ ______________________________ ___________________________ [7] : (ii) The reaction in (c)(i) is a redox reaction. Explain in terms of electrons what this means as applied to this reaction. (You may use ionic equations to help answer this question). ______________________________ ______________________________ ___________________________ [7]

(ii) The reaction in (c)(i) is a redox reaction. Explain in terms of electrons what this means as applied to this reaction. (You may use ionic equations to help answer this question). Zinc [1] loses electrons [1] to form zinc ions or Zn ? Zn2+ + 2e [1] and is oxidised/ions [1] gain electrons [1] to form copper atoms or Cu2 + + 2e ? Cu [1] and is reduced/gain of electrons is reduction [1] reduction and oxidation is redox [1] : (ii) The reaction in (c)(i) is a redox reaction. Explain in terms of electrons what this means as applied to this reaction. (You may use ionic equations to help answer this question). Zinc [1] loses electrons [1] to form zinc ions or Zn ? Zn2+ + 2e [1] and is oxidised/ions [1] gain electrons [1] to form copper atoms or Cu2 + + 2e ? Cu [1] and is reduced/gain of electrons is reduction [1] reduction and oxidation is redox [1]

d) Zinc can be obtained in the laboratory from zinc sulphate solution by displacement with a metal X according to the equation: X + ZnSO4 ? XSO4 + Zn(i) What is the valency of metal X? __________________________ [1] : d) Zinc can be obtained in the laboratory from zinc sulphate solution by displacement with a metal X according to the equation: X + ZnSO4 ? XSO4 + Zn(i) What is the valency of metal X? __________________________ [1]

d) Zinc can be obtained in the laboratory from zinc sulphate solution by displacement with a metal X according to the equation: X + ZnSO4 ? XSO4 + Zn(i) What is the valency of metal X? 2 (allow +2) [1] : d) Zinc can be obtained in the laboratory from zinc sulphate solution by displacement with a metal X according to the equation: X + ZnSO4 ? XSO4 + Zn(i) What is the valency of metal X? 2 (allow +2) [1]

(ii) Suggest one metal which could be used as metal X. ___________________________ [1](iii) Why should sodium not be used in this displacement reaction? ___________________________ [1] : (ii) Suggest one metal which could be used as metal X. ___________________________ [1](iii) Why should sodium not be used in this displacement reaction? ___________________________ [1]

(ii) Suggest one metal which could be used as metal X. Calcium/magnesium [1](iii) Why should sodium not be used in this displacement reaction? Too reactive/dangerous [1] : (ii) Suggest one metal which could be used as metal X. Calcium/magnesium [1](iii) Why should sodium not be used in this displacement reaction? Too reactive/dangerous [1]

e) Heated zinc reacts with steam to produce a gas can be collected using the apparatus shown below. : e) Heated zinc reacts with steam to produce a gas can be collected using the apparatus shown below.

(i) Complete the missing labels A, B and C on the diagram above. [3](ii) Write a balanced symbol equation for the reaction of zinc with steam. ___________________________ [2] : (i) Complete the missing labels A, B and C on the diagram above. [3](ii) Write a balanced symbol equation for the reaction of zinc with steam. ___________________________ [2]

(i) Complete the missing labels A, B and C on the diagram above. [3](ii) Write a balanced symbol equation for the reaction of zinc with steam. Zn + H2O ? ZnO + H2 [2] : (i) Complete the missing labels A, B and C on the diagram above. [3](ii) Write a balanced symbol equation for the reaction of zinc with steam. Zn + H2O ? ZnO + H2 [2]

f) Zinc chloride solution is used to preserve wooden fences. Describe a chemical test that you would carry out to confirm that a sample of wood preservative contained zinc ions. State the observations for a positive test. : f) Zinc chloride solution is used to preserve wooden fences. Describe a chemical test that you would carry out to confirm that a sample of wood preservative contained zinc ions. State the observations for a positive test.

f) Zinc chloride solution is used to preserve wooden fences. Describe a chemical test that you would carry out to confirm that a sample of wood preservative contained zinc ions. State the observations for a positive test. Add sodium hydroxide/ammonia (solution)/ammonium hydroxide [1] white [1] ppt [1] excess [1] ppt redissolves/solution [1] : f) Zinc chloride solution is used to preserve wooden fences. Describe a chemical test that you would carry out to confirm that a sample of wood preservative contained zinc ions. State the observations for a positive test. Add sodium hydroxide/ammonia (solution)/ammonium hydroxide [1] white [1] ppt [1] excess [1] ppt redissolves/solution [1]

Slide 279 : 279 Thanks for viewing. Do consider using others in this Series. Atomic Structure and Bonding. Inorganic: Metal Chemistry Inorganic: Non-metal Chemistry Redox and Electrolytic Chemistry Organic Chemistry Hard Water Acids Bases & Salt Preparations Kinetics and Energetics Miscellaneous Also, check back on this video-lesson from time-to-time during the duration of your course. F Scullion