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Jing Ting Ng Chemistry Year 4 Inglés 40 fichas

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  1. 1Which chemicals (solutions) are colourless?Dilute acids, alkalis; solutions of Gp 1, 2, 3 metals
  2. 2Which chemicals (precipitates) are white?Solid salts of sodium, potassium, ammonium, calcium, zinc (ii), lead (ii) and aluminium (iii)
  3. 3Which chemicals (solids) are grey?Metals in powder form
  4. 4Which chemicals are green?Iron (ii) salts
  5. 5Which chemicals (solids) are blue?Hydrated copper (ii) salts
  6. 6Which chemicals (concentrated solutions) are yellow/brown?Solutions of iron (iii) salts
  7. 7Which chemicals are yellow?Lead (ii) iodide, silver iodide
  8. 8Which chemicals are pale pink?Manganese (ii) salts (undergoes a redox reaction)
  9. 9Which chemicals are purple?Potassium permanganate (redox reaction - oxidising agent)
  10. 10List the cations that may be tested. There are 8 of them.Calcium (ii), zinc (ii), aluminium (ii), lead (ii), magnesium (ii), copper (ii), iron (ii), iron (iii)
  11. 11List the anions that may be tested. There are 6 of them.Carbonate, sulphite, sulphate, chlorine, iodine, nitrate
  12. 12List the gases that may be tested. There are 7 of them.Ammonia, carbon dioxide, chlorine, water vapour, sulphur dioxide, oxygen, hydrogen
  13. 13Which salts are soluble in water?- Gp 1, 2 and ammonium salts
    - Nitrates
    - Hydrogencarbonates
    - Sulphates (EXCEPT LEAD, BARIUM AND CALCIUM SULPHATES, though calcium sulphate is slightly soluble)
    - Chlorides, Bromides and Iodides (except lead and silver)
  14. 14Which salts are insoluble in water?- Carbonates
    - Hydroxides
    - Oxides
    - Sulphides and sulphites
    (EXCEPT GP 1, 2 AND AMMONIUM SALTS. Calcium salts are slightly soluble.)
  15. 15Which cations are insoluble in a little aqeous NaOH?NIL.
  16. 16Which cations are soluble in a little aqeous NaOH?- Ca^2+ (white precipitate)
    - Zn^2+ (white precipitate)
    - Al^3+ (white precipitate)
    - Pb^2+ (white precipitate)
    - Mg^2+ (white precipitate)
    - Cu^2+ (blue precipitate)
    - Fe^2+ (dirty-green precipitate)
    - Fe^3+ (brown precipitate)
  17. 17Which cations are insoluble in excess aqeous NaOH?- Ca^2+
    - Mg^2+
    - Cu^2+
    - Fe^2+
    - Fe^3+
  18. 18Which cations are soluble in excess aqeous NaOH? Explain the significance of these three cations.- Zn^2+
    - Al^3+
    - Pb^2+
    Metal hydroxides such as these three are amphoteric in nature. In this case, they react with excess aqeous NaOH to form complex salts that are soluble to give colourless solutions.
  19. 19Which cations are insoluble in a little aqeous NH3?- Ca^2+ (no reaction)
    - Zn^2+ (white precipitate)
    - Al^3+ (white precipitate)
    - Pb^2+ (white precipitate)
    - Mg^2+ (white precipitate)
    - Cu^2+ (blue precipitate)
    - Fe^2+ (dirty-green precipitate)
    - Fe^3+ (brown precipitate)
  20. 20Which cations are soluble in a little aqeous NH3?NIL.
  21. 21Which cations are insoluble in excess aqeous NH3?- Mg^2+
    - Al^3+
    - Pb^2+
    - Fe^2+
    - Fe^3+
  22. 22Which cations are soluble in excess aqeous NH3?- Ca^2+
    - Cu^2+
    - Zn^2+
  23. 23Which anions may be identified using dilute acids as reagent?- carbonate ion (set up limewater test - CO2 evolved and forms white precipitate with calcium hydroxide solution)
    - sulphite ion (add a few drops of potassium permanganate or potassium dichromate - SO2 evolved turns purple potassium permanganate colourless, turns orange potassium dichromate green)
  24. 24Which anions may be identified using aqeous barium chloride and hydrochloric acid OR aqeous barium nitrate and nitric acid as reagent?- sulphate ion (no effervescence, white precipitate evolved)
    - carbonate ion (set up limewater test - CO2 evolved and forms white precipitate with calcium hydroxide solution)
    - sulphite ion (add a few drops of potassium permanganate or potassium dichromate - SO2 evolved turns purple potassium permanganate colourless, turns orange potassium dichromate green)
  25. 25Which anions may be identified using aqeous silver nitrate and nitric acid?- iodine ion (yellow precipitate formed)
    - chlorine ion (white precipitate formed on addition of silver nitrate, insoluble in nitric acid)
    - carbonate ion (set up limewater test - CO2 evolved and forms white precipitate with calcium hydroxide solution)
    - sulphite ion (add a few drops of potassium permanganate or potassium dichromate - SO2 evolved turns purple potassium permanganate colourless, turns orange potassium dichromate green)
  26. 26Which anions may be identified using aqeous lead (ii) nitrate?- iodine ion (yellow precipitate formed in boiling water)
    - carbonate and sulphate ions (white precipitate formed)
    **cannot be used to differentiate between carbonate and sulphate ions
  27. 27Which anions may be identified using aqeous NaOH or by adding Devarda's alloy, then warming?- nitrate ion (effervescence observed, evolved nitrogen dioxide turns red litmus paper blue)
  28. 28Name the gas: Brown-coloured, turns red litmus paper blueNO2
  29. 29Name the gas: Yellowish-green, bleaches red litmus paper, or turns blue litmus paper red and THEN bleaches itCl2
  30. 30Name the gas: Colourless, odourless, relights glowing splintO2
  31. 31Name the gas: Colourless, odourless, extinguishes lighted splint with a 'pop' soundH2
  32. 32Name the gas: Colourless, odourless, extinguishes lighted splint, forms white precipitate with limewaterCO2
  33. 33Name the gas: Colourless, odourless, extinguishes lighted splint, no white precipitate formed with limewaterH2O (water vapour)
  34. 34Name the gas: Colourless, pungent smell, turns moist blue litmus paper redSO2
  35. 35Name of gas: Colourless, pungent smell, turns moist red litmus paper blueNH3
  36. 36List the conditions for preparation of salts by reaction of acid with insoluble substance.- salt is soluble in water
    - both starting materials insoluble in water
    - starting materials are NOT group 1 metals or unreactive metals
    - suitable for acid + metal, acid + insoluble base + insoluble carbonate
  37. 37State the procedure for reaction of acid with insoluble substance.1. Fill beaker with acid
    2. Add the metal/base/carbonate slowly with constant stirring, until no more reaction occurs or no more effervescence is observed
    3. Filter to remove excess metal/base/carbonate
    4. Heat filtrate to saturation
    5. Allow saturated solution to cool so salt can crystallise
    6. Filter solution to collect crystals
    7. Wash crystals with a little cold water to remove impurities. Dry crystals between a few sheets of filter paper.
  38. 38List the conditions for preparation of salts by titration.- salt is soluble in water
    - both starting solubles soluble in water
    - suitable for acid + alkali, acid + soluble carbonates
  39. 39List the conditions for preparation of salts by precipitation.- salt is insoluble in water
    - suitable for aqeous solution + aqeous solution
  40. 40State the procedure for precipitation.1. Pour 50cm^3 of reactant 1 into a beaker.
    2. Add reactant 2 in excess.
    3. Stir until no more precipitate forms.
    4. Filter to collect precipitate.
    5. Wash the precipitate with distilled water to remove impurities.
    6. Allow precipitate to dry on a piece of filter paper.

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Year 4 Chemistry Fichas sobre SPA, creado por Jing Ting Ng el 26/08/2018.
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Jing Ting Ng
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