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Chemistry Paper 1 - Coggle Diagram

- - - - Mix the solution containing the insoluble solid and the solvent then add a filter funnel to the top of the beaker and add filter paper to said funnel. Once this has been done pour the solution through the filter paper and the solid will be kept at the top as residue and a pure solution of the solvent will be collected at the bottom.
    - - First, pour the solution into an evaporating dish and heat it using a Bunsen burner.Stop heating it when crystals start to form ('point of crystallisation') and allow it to cool down.Then either leave it to allow the rest of the water to evaporate, or filter out the crystals using filter paper and a funnel. Lastly, dry the crystals in a warm oven.Then either leave it to allow the rest of the water to evaporate, or filter out the crystals using filter paper and a funnel. Lastly, dry the crystals in a warm oven.
  - - - Firstly, heat the solution in a boiling flask and once the boiling point of one of the liquids is reached, the liquid will evaporate and travel up the fractionating column where its coolest at the top. The gas will condesne and travel through the condenser as a seprate liquid and will be collected by one of the beakers
      - Simple distillation uses liquids with very different boiling points
      - Fractional distillation uses liquids with similar boiling points i.e. Salt water and pure water
  - - - From Group 3 - Group 5 they can form ions with multiple charges, they are hard and often they form coloured compounds as well as this they are used as catalysts. They are also denser and have high mp and bp
    - - Group 1 metals, they are soft but very reactive as they only need to lose one electron from their outer shells. They have high mp and bp and the reactivity increases as you move down the group.
  - - - Found in group, they form negative ions their bp and mp increase as you move down the group but their reactivity decreases. They also exist as diatomic molecules
    - - Inert because they have full outer shells so they don't need to partake in chemical reactions, they are not flammeable but their bp and mp increases as you go down the group
- - - - Breaking bonds require energy so therefore it's endothermic
      - Forming bonds releases energy so it's exothermic
- - - - By using a universal indicator you can see what colour a substance is, acids are red
    - - Neutral substances are green
    - - Alkaline substances are blue/purple
    - - Alkalis are soluble bases, all alkalis are bases but not all bases are alkali
  - - - Part 1
      - Place dilute acid in a beaker and heat gently.
      - Add the solid base bit by bit until it stops reacting, which means it's in excess.
      - Isolate the salt solution by filtering out the excess solid base using filter paper and a funnel.
      - Part 2
      - Heat the salt solution gently in a water bath until crystals start to form.
      - Let the solution cool further, which will cause more crystals to precipitate.
      - Filter out the soluble salt crystals using filter paper and funnel.
  - - - Bromine is attracted to the anode, becomes discharged (loses its ions) and forms bromine gas
      - Lead gains the ions that travel through the wire and forms Lead metal which sink to the bottom
      - The electrolyte contains a solution of Lead Bromide (containing lead and bromide ions) in a dissolved ionic state
      - Oxidation reaction = 2Br→Br2- + 2e-
      - Reduction = Pb2 + 2e- → Pb
    - - Electrolysis is used to seperate metals from metal oxides
      - 2Al2O3→ 4Al + 3O2
      - Ions in aluminium are fixed (solid), its found in an ore known as bauxite. We need to turn this into molten aluminium oxide
      - Steps
        
        1.) Purify the bauxite
        
        2.) Melt Al2O3, then mix it with cryolite to lower its m.p and b.p
        
        3.) Still at a very high m.p so require high temperatures (960 degrees)
        
        4.) Electrolyte solution contains Al3+ and O2- ions
        
        5.) The oxygen atoms are attracted to the anode and discharged
        
        6.) Electrons flow through the wire, pushed by the battery and reach the cathode
        
        7.) The Al3+ ions are attracted to the cathode and discharged (gain the electrons from the oxygen)
        
        8.) The oxygen atoms join up and form a oxygen gas
    - - Negative cathode attracts positive ions (Metal and H+)
      - Cathode will discharge the lesser reactive one so: Copper,Gold,Silver,Platinum
      - At the anode its a similar thing, however if a halide ion (F- or Br-) is present then its discharged, if not then its the OH- ion
      - In a dissolved solution, there are the ions that you are trying to extract and the ions from water (H+ and OH-)
      - Electrolysis of CuSO4
        
        Ions: Cu2+ and So4(2-) AND H+ and OH-
        
        Cathode = Copper ions get discharged (as its below hydrogen in the reactivity series) copper accumulates around cathode as a solid
        
        Anode = The hydroxide ions get discharged as there is no halide ions present, hydroxide gives up its electron and forms oxygen and water