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National 5 Chemistry Exam Revision

National 5 Chemistry Exam Revision. Chemical Changes. Reaction Rates. 1. A student investigated the reaction between dilute hydrochloric acid and sodium carbonate. One experiment involved measuring the volume of carbon dioxide produced when solid sodium carbonate was used.

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National 5 Chemistry Exam Revision

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  1. National 5 ChemistryExam Revision Chemical Changes

  2. Reaction Rates

  3. 1. A student investigated the reaction between dilute hydrochloric acid and sodium carbonate.One experiment involved measuring the volume of carbon dioxide produced when solid sodium carbonate was used. a) Calculate the average rate in cm3/s of carbon dioxide produced between 10 and 40 seconds. b) Calculate the average rate in cm3/s of carbon dioxide produced in the first 40seconds. c) When did the reaction finish?

  4. Copy and complete the diagram to show how the carbon dioxide gas could be collected from the reaction of calcium carbonate chips and sulphuric acid.

  5. Atomic Structure & Bonding

  6. The table shows the numbers of protons, electrons and neutrons in four particles, W, X, Y and Z. Which pair of particles are isotopes? A. W and X B. W and Y C. X and Y D. Y and Z

  7. Bromine has two isotopes. One has a mass number of 81 and the other has a mass number of 79. The relative atomic mass of bromine is 80. What does this tell you about the percentage of each isotope in bromine? Chlorine has two isotopes. One has a mass number of 35 and the other has a mass number of 37. The relative atomic mass of chlorine is 35.5. Which isotope of chlorine is most abundant in the sample?

  8. Find the number of protons, neutrons and electrons in each of the following; 1. 2. 3. 4.

  9. Which substance exists as diatomic molecules • Sodium chloride • Nitrogen monoxide • Silicon tetrachloride • Sulfur dioxide Solid ionic compounds do not conduct electricity because; • The ions are not free to move • The electrons are not free to move • Solid substances never conduct electricity • There are no charged particles in ionic compounds

  10. Draw a diagram to show how the outer electrons are shared in a molecule of; • Hydrogen chloride • Hydrogen sulfide • Nitrogen fluoride • Water • Methane

  11. Which of the following diagrams could be used to represent the structure of a covalent network?

  12. The table gives information about some substances. • Identify the two ionic compounds. • Identify the covalent network • Identify the covalent molecular compound • Identify the substance which is a gas at room temperature (210C)

  13. A substance X, has a melting point of 996⁰C and a boiling point of 1704⁰C. It only conducts electricity when molten or when dissolved in water. The structure of X is likely to be • Ionic • Metallic • Covalent network • Covalent molecular

  14. Formula and reactant quantities

  15. Write the chemical formula for; • Sodium fluoride • Magnesium carbide • Calcium carbonate • Potassium permanganate • Cobalt (II) chloride • Ammonium nitrate

  16. Write the ionic formula for; • Lithium iodide • Magnesium oxide • Copper (II) carbonate • Calcium sulphite • Beryllium hydroxide • Ammonium phosphate

  17. In vanadium oxide, VaO2, what is the valency of vanadium? A 1 B 2 C 3 D 4 What is the charge on the chloride ion in SnCl4? A 1+ B 1– C 4+ D 4–

  18. Acids & Alkalis

  19. Precipitation is when two solutions react to form an insoluble product. Which of the following pairs of solutions would react together to produce a precipitate? • Silver (I) nitrate + sodium chloride • Copper (II) sulphate + sodium nitrate • Magnesium chloride + lithium nitrate • Barium chloride + potassium nitrate When barium nitrate solution is mixed with sodium sulphate solution, the name of the precipitate formed is • barium chloride • barium sulphate • sodium chloride • sodium nitrate

  20. Which of the following gases would dissolve in water to produce an alkaline solution? • Carbon dioxide • Nitrogen dioxide • Ammonia • Methane Which of the following oxides would dissolve in water to produce an acidic solution? (You may wish to consult your data booklet) • sulphur dioxide • iron (III) oxide • copper (II) oxide • sodium oxide

  21. Which of the following is not a salt? • Sodium chloride • Lithium sulphate • Potassium hydroxide • Copper (II) nitrate Which of the following reactions would not result in the formation of a salt? • Acid + alkali • Acid + reactive metal • Acid + alcohol • Acid + carbonate

  22. Name the product (s) of the following neutralisation reactions; • Magnesium and hydrochloric acid • Potassium hydroxide and sulfuric acid • Magnesium carbonate and hydrochloric acid • Calcium carbonate and nitric acid • Ammonia and sulfuric acid

  23. Which of the following statements correctly describes the concentration of H+ (aq) and OH- (aq) ions in an acidic substance when compared to pure water? The concentration of H+ (aq) and OH- (aq)ions are zero. The concentration of H+ (aq) and OH- (aq)ions are equal. The concentration of H+ (aq) is higher than OH-(aq) ions. The concentration of H+ (aq) is lower than OH- (aq) ions.

  24. Which line in the table correctly describes what happens to a dilute solution of hydrochloric acid when water is added to it?

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