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Chemistry > Metals and their extractions > Flashcards

Metals and their extractions Flashcards

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1
Q

What are metals extracted from and where are they found?

A

Metals are extracted from ores which is a substance found in the Earth’s crust which contains metal compounds.

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2
Q

How can metals be extracted?

A

Metals can be extracted from their ores by chemical reactions or electrolysis.

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3
Q

What does the reactivity of a metal tell you?

A

The more reactive a metal is, the more stable its compound is so it’s harder to extract pure metal.

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4
Q

How are metals MORE reactive than carbon extracted?

A

Electrolysis

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5
Q

How do displacement reactions work?

A

Any metal can displace a metal lower than itself in the reactivity series from a solution of one of its salts. A displacement reaction is when a more reactive metal displaces a less reactive metal from a compound.

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6
Q

What is reduction?

A

The removal of oxygen atoms from a chemical or the gain of electrons.

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7
Q

What is oxidation?

A

The addition of oxygen atoms to a chemical or the loss of electrons.

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8
Q

What does OILRIG stand for?

A

Oxidation Is the Loss of electrons Reduction Is the Gain of electrons.

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9
Q

What is a redox reaction?

A

A reaction where both reduction and oxidation occur

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10
Q

What are the raw materials for the extraction of iron and what are they use for?

A

Iron ore - Source of iron
Coke - Used as a fuel and to produce carbon monoxide for the reduction
Limestone - To remove impurities
Hot air - Provides oxygen so that coke can burn

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11
Q

What is the first step of extracting metals from their ores?

A

Combustion - The coke burns on the air.
Carbon + Oxygen -> Carbon Dioxide
C + O₂ -> CO₂

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12
Q

What is the second step of extracting metals from their ores?

A

Oxygen from the hot air reacts with coke (carbon) to form carbon monoxide. This is an exothermic reaction (combustion).
Carbon + Oxygen -> Carbon monoxide
2C + O₂ -> 2CO

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13
Q

What is the third step of extracting metals from their ores?

A

The carbon monoxide reacts with the iron ore, forming molten iron. This is a reduction reaction.
Iron oxide + Carbon monoxide -> Iron + Carbon Dioxide
Fe₂O₃ + 3CO -> 2fe +3CO₂

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14
Q

What is the fourth step of extracting metals from their ores?

A

The added limestone thermally decomposes in the heat of the furnace (decomposition).
Calcium carbonate -> Calcium Oxide + Carbon Dioxide
CaCO₃ -> CaO + CO₂

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15
Q

What is the final step of extracting metals from their ores?

A

The calcium oxide reacts with acidic impurities (silicon dioxide) in a neutralisation reaction.
Calcium oxide + Silicon dioxide -> Calcium silicate (Slag)
CaO + SiO₂ -> CaSiO₃

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16
Q

What are the steps of the extraction of iron?

A

Combustion - Reduction - Decomposition - Neutralisation

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17
Q

Where is aluminium in the reactivity series?

A

Aluminium is higher than iron and carbon in the reactivity series.

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18
Q

Why can’t aluminium be extracted like other metals below it in the reactivity series?

A

So much energy is needed to extract it from its ores and reduction/oxidation reductions involving carbon cannot be used.

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19
Q

How is aluminium extracted?

A

Aluminium and higher metals in the reactivity series are extracted using electrolysis.

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20
Q

What must be done to aluminium before it’s extracted?

A

Aluminium oxide is heated to high temperatures making it melt so electricity can pass through it.

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21
Q

What happens when aluminium is extracted?

A

Positively charged aluminium ions move towards the negatively charged cathode forming aluminium atoms that can be extracted as aluminium metal. Oxygen forms at the positive electrode and it reacts with the carbon forming carbon dioxide which bubbles out of the tank.

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22
Q

What is the negatively charged rod called?

A

Cathode

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23
Q

What is the positively charged rod called?

A

Anode

24
Q

What are the negatively charged atoms called?

A

Anions

25
Q

What are the positively charged atoms called?

A

Cations

26
Q

What are the problems with extraction of metals?

A

The melting point of aluminium oxide is very high which makes it expensive to melt.
Greenhouse gas emissions
Effect on local environment and population

27
Q

How can you reduce the melting point of aluminium oxide?

A

Aluminium oxide is dissolved in a substance called cryolite which lowers the melting point. The use of molten cryolite as a solvent reduces some of the energy costs involved in extracting aluminium.

28
Q

What can happen to the positive electrode after a while?

A

As the positive electrode itself reacts with oxygen the positive electrode gradually burns away so the positive electrode has to be replaced often

29
Q

What is electrolysis?

A

Electrolysis is a chemical reaction involving the splitting up of a compound using an electrical current passing through a conducting liquid.

30
Q

What does the electrolyte contain?

A

Positively charged ions called cations and negatively charged ions called anions.

30
Q

What happens during the electrolysis of molten salts?

A

When the electrolyte contains only two ions the positive ions will go to the cathode and negative ions go to the anode.

30
Q

What is the conducting liquid called?

A

The electrolyte

30
Q

What happens at the cathode during the electrolysis of aqueous salts?

A

At the cathode hydrogen is produced unless the + ions in the ionic compound are from a metal less reactive than hydrogen. If the metal is less reactive it will be produced instead.

30
Q

What ions are in aqueous salts?

A

When you have an ionic solution your solution will contain the ions that make up the ionic compound and the ions in water (OH- and H+)

31
Q

What happens at the anode during the electrolysis of aqueous salts?

A

At the anode oxygen will be produced unless the ionic compound contains halide ions (Chlorine, bromine, iodine)

32
Q

What can the electrolysis of water be used for?

A

Electrolysis can be used to separate water into hydrogen gas and oxygen gas.

33
Q

What is the equation for electrolysis of water?

A

2H₂O -> 2H₂ + O₂
Water -> Hydrogen + Oxygen

34
Q

What is the reaction that occurs at the anode during the electrolysis of water?

A

An oxidation reaction occurs
4OH- -> 2H₂O + O₂ +4e-

35
Q

What is the reaction that occurs at the cathode during the electrolysis of water?

A

At the cathode a reduction reaction occurs.
4H+ + 4e -> 2H₂

36
Q

What are the transition metals?

A

The transition metals are the metallic elements found in the centre of the periodic table.

37
Q

What physical and chemical properties do transition metals have?

A

Malleable
High melting and boiling points
Good conductors of heat and electricity
FORMS COLOURED COMPOUNDS

38
Q

What is the result for Cu2+ when sodium hydroxide is added?

A

Blue precipitate of Cu(OH)₂

39
Q

What is the result for Fe2+ when sodium hydroxide is added?

A

Green/grey precipitate of Fe (OH)₂

40
Q

What is the result for Fe3+ when sodium hydroxide is added?

A

Rust brown precipitate of Fe(OH)₃

41
Q

What is the ion when silver nitrate is added to it and a white precipitate is formed?

A

Chlorine

42
Q

What is the ion when silver nitrate is added to it and a cream precipitate is formed?

A

Bromine

43
Q

What is the ion when silver nitrate is added to it and a yellow precipitate is formed?

A

Iodine

44
Q

What properties does iron (steel) have?

A

Malleable
Good conductor of heat and electricity
Steel is harder and stronger than iron and less likely to rust

45
Q

What uses does iron (steel) have?

A

Magnets, railway lines, cutlery

46
Q

What properties does aluminium have?

A

Low density
Light weight
Strong
Resists corrosion

47
Q

What uses does aluminium have?

A

Aircraft, saucepans, drink cans

48
Q

What properties does copper have?

A

Good conductors of heat and electricity
Malleable
Ductile

49
Q

What uses does copper have?

A

Copper wires, saucepan bottoms

50
Q

What properties does titanium have?

A

Hard and strong
Low density
High melting and boiling point
Resistant to corrosion

51
Q

What uses does titanium have?

A

Jet engines, medical implants, jewelley

52
Q

What is an alloy?

A

An alloy is a mixture of 2 or more different metals (or carbon) made by combining the molten metals.

Chemistry (6 decks)

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