2.3 Metals & Their Extractions Flashcards
Displacement Reaction
When a more reactive element replaces a less reactive element in a compound eg: Magnesium and Copper Sulfate - less reactive can’t push the other out
Below Carbon on reactivity Series
Can be extracted by heating with carbon - reduction (oxygen removed) and anything above needs electrolysis
Extracting Iron in a Blast Furnace
Iron Oxide + Carbon Monoxide ——> Iron + Carbon Dioxide
Raw Materials
In the top of the blast furnace they put in iron ore, limestone and coke and at the bottom you put hot air
Stage 1
Hot air reacts with Coke producing heat and carbon monoxide gas
Stage 2
Carbon Monoxide reacts with Iron and Carbon Dioxide floats down and is taken out (turned into steel)
Fe2O3 + 3CO ——> 2Fe + 3CO2
Stage 3
Limestone reacts with acidic impurities (sand and shingle) making Slag or Calcium Silicate (used in roads)
CaCO3 + SiO2 ——> CaSiO3
Electrolysis
Splitting up a compound into its elements by addition of electricity
Aluminium Oxide 2Al2O3 ——> 4Al + 3O2
Copper Sulfate Cu + 2e ——> Cu
PANCAKE
Posative anode, negative cathode
Aluminium Oxide in Electrolysis
Al is a positive ion and will travel to the negative cathode, while oxygen is negative and will travel to the positive anode as opposites attract
OARC
Oxidation at the anode, Reduction at the cathode
OILRIG
Oxidation is loss of electrons, Reduction is gain of electrons
Electrodes
They are made of graphite and it HOT Oxygen will react making Co2 and you have to replace the positive electrode a lot
To save money people
Put Aluminium with Cryolite to reduce Al high melting point to save money
Ore
Compound of metals mixed with impurities in the earth crust