C3 Knowledge Test – Higher Tier

  1. Why was Mendeleev’s periodic table accepted, where Newland’s was not?
  2. How did Mendeleev decide on the order of the elements in the periodic table?
  3. What is the modern periodic table arranged by?
  4. Why do elements in the same group have similar properties?
  5. Write a word and symbol equation for the reaction of a group 1 metal with water.
  6. How would you expect the reactivity of rubidium to compare with lithium. Explain your reason.
  7. Write a word and symbol equation for a group 7 element with a group 1 element.
  8. How and why does reactivity change within the halogen group?
  9. Name five ways transition elements differ to group 1 metals?
  10. What causes water to be ‘hard’?
  11. What forms when hard water reacts with soap?
  12. Describe the health benefits of hard water.
  13. Describe two ways in which permanent hardness can be removed.
  14. What is the difference between ‘pure’ water and ‘drinking’ water?
  15. Why is chlorine added to drinking water?
  16. What do each of the symbols in Q = mc ΔT stand for?
  17. Define ‘exothermic change’ and ‘endothermic change’.
  18. What sort of reaction is represented by this energy level diagram?
  19. What sort of reaction is this, what is represented by ‘X’?
  1. Describe what happens to bonds in exothermic and endothermic reactions.
  2. Describe how a catalyst works, in terms of energy.
  3. Give an advantage and a disadvantage of hydrogen fuel cells.
  4. What colour flame will the following ions burn with; K+, Na+, Ca2+, Ba2+, Li+?
  5. What colour precipitate is formed when sodium hydroxide is added to; Al3+, Cu2+, Mg2+, Fe2+, Fe3+, Ca2+?
  6. How can you distinguish between Al3+, Mg2+ and Ca2+ ions?
  7. Describe the test for carbonate ions.
  8. Write a word and symbol equation (with state symbols) for the reaction between silver nitrate and sodium chloride.
  9. What colours are the three silver halides?
  10. Why do we not use hydrochloric acid to acidify the silver nitrate?
  11. What do we add to solutions to test for sulphate ions?
  12. Give two reasons why barium sulphate is given as a barium meal.
  13. What is an ‘end point’?
  14. 25.00cm3 of sodium hydroxide solution was pipetted into a conical flask. It was titrated against 0.10mol/dm3 hydrochloric acid. The mean volume of acid needed was 24.00cm3.

(a)Write the balanced equation for the reaction

(b)Calculate the concentration of sodium hydroxide used in the titration above.

  1. What are the raw materials of the Haber process, where do we get them from?
  2. What are the conditions of the Haber process?
  3. What does this symbol: mean?
  4. What are two conditions of equilibrium?
  5. How does raising the temperature of the Haber process affect the yield and the rate?
  6. Why does raising the temperature have these effects?
  7. Why does increasing the pressure of the Haber process increase the yield?
  8. What are the structural and displayed formulae of ethanol? Highlight the functional group.
  9. Name the first three molecules in the alcohols’ homologous series.
  10. Write a balanced symbol equation for the complete combustion of propanol in air.
  11. Name at least three uses of alcohols.
  12. What is the process that turns ethanol into ethanoic acid?
  13. What are the structural and displayed formulae of ethanoic acid? Highlight the functional group.
  14. What would happen if a carboxylic acid came into contact with a carbonate?
  15. Describe the difference between a ‘weak’ acid and a ‘strong’ acid.
  16. What is the functional group of the esters?
  17. What is the name of this compound: , what is its structural formula?