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5.5 explain the uses of aluminium and iron, in terms of their properties

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5.5 explain the uses of aluminium and iron, in terms of their properties

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Aluminium: aeroplane bodies, overhead power cables, saucepans, food cans, window frames.
- high strength-to-weight ratio
- good conductor of electricity
- good conductor of heat
- non-toxic
- resists corrosion

Iron: car bodies, iron nails, ships, bridges
- strong

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1.55 - write ionic half equations representing the reactions at the electrodes during electrolysis

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1.55 - write ionic half equations representing the reactions at the electrodes during electrolysis

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Na+ + e- ==> Na
2Cl- ==> Cl2 + 2e-

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5.3  write ionic half-equations for the reactions at the electrodes in aluminium extraction

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5.3  write ionic half-equations for the reactions at the electrodes in aluminium extraction

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Al³⁺ + 3e⁻ ➝ Al(l) (Cathode & reduced)

2O²⁻ ➝ O₂ + 4e⁻ (Anode & oxidised)

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1.53 - describe experiments ot investigate electrolysis using inert electrodes of molten salts such as lead (II) bromide and predict the product

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1.53 - describe experiments ot investigate electrolysis using inert electrodes of molten salts such as lead (II) bromide and predict the product

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lead forms at cathode
bromine forms at anode

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1.50 - understand why ionic compounds conduct electricity only when in molten or in solution

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1.50 - understand why ionic compounds conduct electricity only when in molten or in solution

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ionic compounds have oppositely charged ions that are mobile in aqueous & molten states, able to ensure a flow of electric charges

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2.29 understand that metals can be arranged in a reactivity series based on the reactions of the metals and their compounds

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2.29 understand that metals can be arranged in a reactivity series based on the reactions of the metals and their compounds

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Potassium
Sodium
Lithum
Calcium
Magnesium
Aluminium
Zinc
Iron
Copper
Silver
Gold

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1.51 - describe experiments to distinguish between electrolytes and non-electrolytes

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1.51 - describe experiments to distinguish between electrolytes and non-electrolytes

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make an electric circuit with a break in the wire. when you put both ends in a solution and the LED lights up, the current flows -- electrolyte

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1.52 - understand that electrolysis involves the formation of new substances when ionic compounds conduct electricity

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1.52 - understand that electrolysis involves the formation of new substances when ionic compounds conduct electricity

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cations attracted to cathode
anions attracted to anode

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1.54 - describe experiments to investigate electrolysis, using inert electrodes, of aqueous solutions such as sodium chloride, copper (II) sulphate and dilute sulphuric acid and predict the products

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1.54 - describe experiments to investigate electrolysis, using inert electrodes, of aqueous solutions such as sodium chloride, copper (II) sulphate and dilute sulphuric acid and predict the products

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NaCl - sodium & chlorine
CuSO4 - copper and oxygenlll
H2SO4 dilute - hydrogen and oxygen

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Aluminium Extraction - 






5.2  describe and explain the extraction of aluminium from purified aluminium oxide by electrolysis, including: 
i the use of molten cryolite as a solvent and to decrease the required operating temperature 
ii the need to replace the positive electrodes 
iii the cost of the electricity as a major factor  

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Aluminium Extraction - 






5.2  describe and explain the extraction of aluminium from purified aluminium oxide by electrolysis, including: 
i the use of molten cryolite as a solvent and to decrease the required operating temperature 
ii the need to replace the positive electrodes 
iii the cost of the electricity as a major factor  

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Method: electrolysis
Aluminium ore: Bauxite
Dissolved in molte cryolite to decrease melting point temperature

Expensive because:
- The high temperatures burn the carbon anode forming CO2. They have to be replaced
- Great use of electricity is expensive

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1.48 - understand that an electric current is a flow of electrons / ions

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1.48 - understand that an electric current is a flow of electrons / ions

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5.4 describe and explain the main reactions involved in the extraction of iron from iron ore (haematite), using coke, limestone and air in a blast furnace

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5.4 describe and explain the main reactions involved in the extraction of iron from iron ore (haematite), using coke, limestone and air in a blast furnace

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Oxygen in the air reacts with coke to form carbon dioxide
- C(s) + O2(g) --> CO2(g)

Carbon dioxide reacts with coke to firm carbon monoxide

- CO2(g) + C(s) --> 2CO(g)

Carbon monoxide reduces iron (III) oxide in iron ore
- Fe2O3 + 3CO(g) --> 2Fe(l) + 3CO2(g)

Calcium carbonate in the limestone decomposes to form calcium oxide

- CaCO3(s) --> CaO(s) + CO2(g)

Calcium oxide reacts with silicon dioxide, which is an impurity in iron ore, to form calcium silicate

- CaO(s) + SiO2(s) --> CaSiO3(l)

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5.1  explain how the methods of extraction of the metals in this section are related to their positions in the reactivity series 

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5.1  explain how the methods of extraction of the metals in this section are related to their positions in the reactivity series 

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Higher up reactivity series ➝ electrolysis, then Heat with carbon in blast furnace and lowest ➝ Heat only

| Potassium | Electrolysis
| Sodium | Electrolysis
| Lithium | Electrolysis
| Calcium | Electrolysis
| Magnesium | Electrolysis
| Aluminium | Electrolysis

| Zinc | Heat with carbon, Blast furnace
| Iron | Heat with carbon, Blast furnace
| Copper  | Heat with carbon, Blast furnace

| Silver | Heat only
| Gold | Heat only

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1.49 - understand why covalent compounds do not conduct electricity

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1.49 - understand why covalent compounds do not conduct electricity

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covalent compounds don't have mobile and delocalised electrons so they are unable to ensure flow of electrical charges