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C3 REVISION – CHAPTER 1 – The Periodic Table How did Newlands arrange the elements in his model of the Periodic Table? What was this layout of the elements known as? Why was it largely discredited? What did Mendeleev do differently to Newlands? • Group 1: aka_____________________ Draw the electron structure of the first three elements • • Why is Mendeleev’s model of the Periodic Table now accepted? How can these elements be made stable in terms of electron shells? How do they achieve this? What charge ion do they therefore form? What is different about the density and melting point of the group 1 metals? What two products are formed when they react with water? How are the elements in the Periodic Table arranged now? • • • Why could they not be arranged like this when Mendeleev and Newlands were working? Name the following groups: 1. Group 7: aka_____________________ Draw the electron structure of the first two elements 7. 0. Which group(s) in the Periodic Table contain only metals? Which group(s) in the Periodic Table contain only non-metals? How can these elements be made stable in terms of electron shells? How do they achieve this? What charge ion do they therefore form? What will a more reactive halogen do to an aqueous solution of another halogen salt? Transition Metals Compare the following properties of the transition metals with group 1 metals: Patterns of Reactivity in Group 1 and Group 7 Describe how reactivity changes going down each group. Melting point*: Strength/Hardness: Reactivity: *which metal is the exception? Transition metals can form ions with _____________ charges. They are Group 1 ______________ down the group. Group 7 _____________down the group. useful as _________ and form lots of different _____________ compounds. Explain why reactivity changes going down each group. C3 REVISION – CHAPTER 2 – Water Hard Water How can this experiment be used to determine water hardness? What is hardness in water caused by? Water Quality What should there not be lots of in drinking water? How is water made suitable for drinking? (Main Stages) • • • • How do these substances come to be in water? • • • Two “types” of hard water • • Explain what happens during the following stages •Filtration Why does using hard water cost money? •Sedimentation • • • Explain How the Following Remove ‘Hardness’ • Sodium carbonate (washing soda) What is the purpose of chlorination? What are the benefits of chlorination? • What is soap scum? How is it formed? What is the purpose of adding fluoride to drinking water? Ion Exchange Column What is limescale? How is it formed? List the benefits of using hard water What are the drawbacks of adding fluoride to drinking water? What is the purpose of water filters? Boiling (temporary hard water only) What is distillation of water? Why is it not used to produce pure water? C3 REVISION – CHAPTER 3 – Energy Change What is the unit of energy? What do we call reactions that release energy to the surroundings? Give an example. Use the bond energies from the table to calculate the overall energy change in the Haber process. N2(g) + 3H2(g) What is the equation we use to calculate energy released during reactions? Use the equation above to calculate the energy required to increase the temperature of 50cm3 of water from 21°C to 37°C What do we call reactions that take in energy from the surroundings? Give an example. 2NH3(g) Bond Bond Energy (kJ/mol) N=N 945 H-H 436 N-H 391 Give a definition of a fuel. What do we call the reaction when fuels react with oxygen? Draw an energy level diagram for an exothermic reaction. Is the Haber process endothermic or exothermic going forward? Draw a diagram of the apparatus used to measure energy change in What are the waste products from burning fossil fuels? reactions. What is the waste product from hydrogen fuel cells? Draw an energy level diagram for an endothermic reaction. KEY WORDS: Endothermic Exothermic Calorimeter Reactants Products Bond Energy Hydrogen Fuel Cells ASSESSMENT: C3 REVISION – CHAPTER 4 – Analysis & Quantitative Chemistry TEST FOR POSITIVE IONS State the flame colour produced by the following ions in a flame test. TEST FOR NEGATIVE IONS Describe how you would test for a CARBONATE (CO32- ion). TITRATIONS Describe the main steps in a general titration practical including relevant equipment. Lithium (Li+)____________________ Sodium (Na+)____________________ Potassium (K+)__________________ Calcium (Ca2+)____________________ Barium (Ba2+)_____________________ State the precipitate colour produced by the following ions when they react with OH- ions. Copper II (Cu2+)__________________ Describe how you would test for the following HALIDES Chloride Bromide Iron II (Fe2+)__________________ Iron III (Fe3+)__________________ Iodide Aluminium(Al3+)__________________ Magnesium(Mg2+)__________________ Calcium(Ca2+)__________________ Q. 25cm3 of 0.2M HCl reacts with 22.6cm3 of NaOH of an unknown concentration: calculate the concentration of the NaOH. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) Describe how you would test for the presence of a SULPAHTE (SO42- ion) How would you distinguish between Aluminium, Magnesium and Calcium hydroxides? Aluminium Magnesium Calcium Write out the equation to calculate the number of moles of a substance in solution. KEY WORDS: flame test, sulphate, carbonate, halide, barium chloride, end point, neutralisation, titration ASSESSMENT: C3 REVISION – CHAPTER 5 – Chemical Equlibrium & The Production of Ammonia Explain what is meant when we say a reaction is at equilibrium. The Haber Process N2(g) + 3H2(g) 2NH3(g) – 93kJ/mol What can you say about energy in a reversible reaction? [Think: exo and endothermic] Draw a diagram to describe the main stages in the Haber process. Describe the anhydrous copper sulphate reversible reaction (a diagram may help) State and explain the effect of increasing the pressure in the Haber process above. Use your diagram above to explain how the Haber process is made more efficient in terms recycling unused reactants. State and explain the effect of decreasing the temperature in the Haber process above. Describe how the Ammonia is separated from the unused Nitrogen and Hydrogen. What can anhydrous copper sulphate be used to test for? Describe the reaction conditions for the Haber process above. KEY WORDS: Equilibrium, pressure, forward reaction, reverse reaction, economy, reversible reaction, catalyst ASSESSMENT: Why do we have to compromise with a lower than expected pressure in the Haber process C3 REVISION – CHAPTER 6 – Alcohols; Carboxylic Acids; Esters Draw the structure of a simple alcohol, name it and identify the functional group. Describe the properties of alcohols Describe the properties of carboxylic acids Carboxylic acids are ‘weak’ acids; explain what is meant by a weak acid. Give examples of the uses of alcohols Draw the structure of a simple Carboxylic Acid, name it and identify the functional group. Give examples of the uses of carboxylic acids Describe the problems associated with alcohol consumption in the UK. Describe the properties of esters Give examples of the uses of esters Draw the structure of a simple Ester, name it and identify the functional group. KEY WORDS: Alcohol, carboxylic acid, ester, functional group, solvent, fuel, volatile ASSESSMENT: Describe how you would make an ester.