❌C6.1 (3) - extractions Flashcards
c6.1.6 - extracting metals c6.1.7 - extracting iron c6.1.8 - extracting aluminium c6.1.9 - biological metal extraction
define an ore
a mineral or rock that contains a enough metal/metal compound to make it economical to extract the metal
(= the value of the metal is more than the cost of extracting it)
what is the ore to extract copper (carbonate)?
malechite
what is the ore to extract iron(III) (oxide)?
haematite
what is the ore to extract aluminium (oxide)?
bauxite
describe the 3 main stages to extract a metal
1) ore is mined
2) ore is processed
(metal compound separated from other substances in the ore)
3) metal is extracted from the pure method compound using chemical reactions
what is the mneunomic to remember the metal reactivity series?
(and what does each stand for - in terms of elements)
pink - potassium smiling - sodium cats - calcium meow - magnesium at - aluminium cute - carbon (NOT METAL) zebras - zinc in - iron the - tin long - lead hot - hydrogen (NOT METAL, USED FOR REFERENCE) curly - copper swirly - silver grass - gold privately - platinium
Please stop calling me a (cute) zebra, I think love has copper silver gold platinum
What extraction methods are there - when are they used
- in principle, all metals could be extracted from their compounds using electrolysis, but electricity is expensive
- if metal is less reactive than carbon, cheaper methods are used instead
- copper + iron are less reactive than carbon, so they can be extracted by heating their compounds with carbon or with carbon monoxide
all metals can be extracted from their compounds using …… but is expensive
electrolysis (electricity is expensive)
why can copper be extracted using carbon, but not sodium?
as copper is less reactive than carbon
- wheras sodium is too reactive to be extracted by reduction
describe the 2 main steps of how copper is extracted from copper sulfide
(and the word and symbol equation for each one)
1) copper sulfide (II) is ‘roasted’ in air
(to get it into metal oxide form for carbon to reduce later) :
copper(II) sulfide + oxygen -> copper(II) oxide + sulfur dioxide
2CuS(s) + 3O2 (g) -> 2CuO(s) + 2SO2 (g)
2) copper(II) oxide is heated with carbon:
copper (II) oxide + carbon -> copper + carbon dioxide
2CuO(s) + C(s) -> 2Cu(s) + CO (g)
2
explain how the extraction of copper sulfide is a redox reaction
- and what is the reducing agent
- copper(II) oxide loses oxygen and is reduced
- carbon gains oxygen and is oxidised
- carbon is acting as a reducing agent (reduced copper oxide to copper)
what form of carbon is used when extracting copper from copper sulfide?
charcoal
what is the machinery used to extract iron from its ore called?
a blast furnace
what are the raw materials used to extract iron?
and what is each one’s function
- iron ore (haematite - contains iron needed for extraction)
- coke (reduces iron(III) oxide to iron)
- limestone (purifies iron)
describe the three steps in which iron is extracted
- and the symbol equation for each one
1) coke burns in hot air, making carbon dioxide
C(s) + O (g) -> CO (g)
2 2
2) more coke reduces carbon dioxide to carbon monoxide
C(s) + CO (g) -> 2CO(g)
2
3) carbon monoxide reduces iron(III) oxide to iron
3CO(g) + Fe2O3(s) -> 3CO2 (g) + 2Fe (l)
what is the main reducing agent in the blast furnace for extracting iron from iron(III) oxide?
(and why can it do so)
carbon monoxide
- it is more reactive than iron
in what state does iron leave the blast furnace?
molten state (temperatures are very high, 1500C)
how is extracted iron purified?
- using limestone
1) calcium carbonate decomposes in the high temperatures :
CaCO3(s) -> CaO(s) + CO2(g)
2) calcium oxide reacts with silica from the sandy impurities from extracted iron to form calcium silicate:
CaO(s) + SiO2(g) -> CaSiO3(l)
The molten calcium silicate is called slag. It floats on the molten iron, and both the iron and slag are removed separately at the bottom of the blast furnace.
