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Metal extraction
Chemistry
| Question | Answer |
|---|---|
| An ore... | Is a rock that contains enough of a metal in it for it to be profitable to extract |
| Haematite | Iron ore Fe2O3 |
| Bauxite | Aluminum ore Al2O3 |
| Malachite | Cooper ore |
| Reactivity series: | Potassium Sodium Calcium Magnesium Aluminum Carbon Zinc Iron Tin Lead Hydrogen Copper Silver Gold |
| Above carbon in series uses.... | Electrolysis |
| Between Carbon and Hydrogen uses.... | Blast furnace |
| Under hydrogen..... | Found native |
| Displacement | More reactive elements can displace a less reactive element from a compound |
| Alloy | An alloy is a mixture of a metal and an element which has metallic properties that differ from just the metal structure. |
| Alloy examples: -Bronze -Brass -Solder -Amalgram -Gold | Bronze is copper and tin Brass is copper and zinc- does not tarnish Solder is zinc and iron -used for circuit boards Amalgam is mercury and silver- used for fillings as does not rust Pure gold is soft so ass copper and silver to solidify it |
| REDOX reactions | Reduction and oxidation Reduction is the gain of electrons Oxidation is the loss of electrons OIL RIG |
| Blast furnace | Iron is extracted from haematite in a reduction reaction 1) Hot air reacts with coke to produce heat and carbon dioxide 2) More coke is added to make carbon monoxide for the reduction 3) Haematite is added and iron is produced |
| Impurities in blast furnace | Calcium Carbonate is added to remove the silica impurities |
| Blast furnace equations: | 1) C + O2 -> CO2 2) CO2 + C -> 2 CO 3) Fe2O3 +3CO -> 2 Fe +3CO2 4) CaCo3 -> CaO + CO2 CaO + SiO2-> CaSiO3 |
| Uses of metal -Copper | - Very good conductor -Malleable -Ductile Used for wires |
| Uses of metal -Aluminium | - Good conductor - Strong -High tensile strength - Low density - No corrosion So used for overhead power cables, car parts, saucepans and window frames |
| Uses of metal - Titanium | - Hard -Strong -Corrosion resistant -Low density -High melting point Used for engine parts, medical implants and jewellry. |
| Electrolysis | Used to separate elements in insoluble ionic compounds An electrolyte contains an ionic compound on dissolved or molten form so the ions can freely move Anode is positive and attracts negative ions whilst Cathode is negative and attracts positive ions |
| Copper electrolysis | Copper is purified by splitting Cooper Chloride Chloride goes to anode and is oxidised whilst Copper is reduced at the cathode |
| Aluminium electrolysis | 1) Aluminum Oxide is purified from Bauxite 2) Cryolite is added to reduce melting ​point 3) Aluminium Oxide is melted At anode-> 2O2- > O2+4e- At Cathode-> Al3+ +3e- -> Al Overall-> 2Al2O3 -> 4Al + 3O2 |
| Electrolysis of water | Pure water is not a good conductor so minerals are added 2H20-> 2H2 +O2 At anode= 4OH- -> 2H2O +O2+4e- At cathode= 4H+ +4e-> 2H2 |
| Brine | A highly concentrated solution of sodium chloride |
| Electrolysis rules | If metal is more reactive than Hydrogen then Hydrogen will be produced If a halogen is present the is will be discharged but otherwise Oxygen will be discharged |
Created by:
Zoe 1
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