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Chemistry unit 2 GCSE > Topic 3 Metals and their extraction > Flashcards

Topic 3 Metals and their extraction Flashcards

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1
Q

Where are metals extracted from

A

Metals are extracted from their ores which are minerals found in the earths crust that contain metal compounds

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2
Q

Which metal is the most reactive?

A

Potassium

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3
Q

Which metal is the least reactive?

A

Gold

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4
Q

What does the term native mean and give 2 examples of native elements

A

Native means not joined with other elements and gold and silver are native

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5
Q

The more reactive a metal is, the more ______ its metal compound is so the _____ it is to extract pure metal

A

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

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6
Q

What are the 2 main extraction methods?

A

Electrolysis and Reduction

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7
Q

What are metals above carbon in the reactivity series extracted by?

A

By electrolysis

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8
Q

What are metals below carbon in the reactivity series extracted by?

A

By using carbon and reduction

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9
Q

Why are displacement reactions used?

What happens during this process?

A

Used to extract metals from metal compounds and the more reactive metal will push out the least reactive metal

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10
Q

Give an example of a displacement reaction

A

Magnesium + copper nitrate —-> Magnesium nitrate + copper

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11
Q

Is adding magnesium to copper sulphate a displacement reaction? Give the word and chemical equation as well

A

Yes because magnesium pushes out the copper

Magnesium + copper sulphate —> magnesium sulphate + copper

Mg + CuSO4 —> MgSO4 + Cu

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12
Q

What is oxidation?

A

Oxidation is adding oxygen

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13
Q

What is reduction?

A

Reduction is taking oxygen

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14
Q

Is oxidation a loss or gain of electrons?

A

Oxidation is a loss of electrons

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15
Q

Is reduction a loss or gain of electrons?

A

Reduction is a gain of electrons

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16
Q

What does OILRIG stand for

A 
Oxidation
Is
Loss of electrons
Reduction
Is
Gain of electrons
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17
Q

What is the thermite reaction?

Name what is oxidised and reduced

Give the chemical formula

Is this a endothermic or exothermic reaction?

A

Iron (III) oxide + aluminum —> Iron + aluminium oxide

The aluminum is oxidised and the iron is reduced

Fe2O3 + 2Al —> 2Fe + Al2O3

Exothermic reaction (releases a lot of heat energy)

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18
Q

The species that is reduced is known as what?

A

Oxidising agent

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19
Q

The species that is oxidised is known as what?

A

Reducing agent

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20
Q

What is a redox reaction

A

Where oxidation and reduction both occur

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21
Q

How does a blast furnace work? [6 MARKS]

A
  1. Raw materials (Iron ore, carbon rich coke and limestone) are added to the top of the furnace

2.Hot air is blown to the bottom of the furnace. This allows the oxygen from the blasts of air to react with the carbon in the coke to form CO2. This reaction is exothermic and heats up the furnace
Oxygen + carbon —> carbon dioxide
O2 + C —> C02

This then reacts further to produce Carbon Monoxide. This helps reduce the ore and is a very exothermic reaction. The carbon is reduced
Carbon dioxide + carbon —> carbon monoxide
CO2 + C —> 2CO

  1. As the carbon monoxide rises up the furnace (2CO), it reacts with the iron ore and reduces it to iron
    Iron (III) oxide + carbon monoxide —> Iron + carbon dioxide
    Fe203 + 3CO —> 2Fe + 3CO2
  2. The molten iron collects at the bottom of the furnace and it is about 96% pure - called cast iron

5.The limestone reacts with the impurities (lots of sand) to form slag. This floats on top of the iron and is drained off
Calcium carbonate —> Calcium oxide + carbon dioxide
CaCO3 —> CaO + CO2

6.The reactions inside the furnace produce carbon dioxide and nitrogen. these gases are removed from the gas outlet

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22
Q

What is neutralisation and give an example of a neutralisation reaction

A

Neutralisation is the reaction between an acid and a base to form a salt plus water.
Example - Calcium oxide + silica —> calcium silicate

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23
Q

What is electrolysis

A

Electrolysis is the process of splitting a compound up by using electricity

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24
Q

To conduct electricity we have to have ________ compounds because they conduct electricity when you _____ or _____ them

A

Have to have ionic compounds because they conduct electricity when you melt or dissolve them

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25
Q

What is an electrolyte?

A

The substance being broken down

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26
Q

What are the positive and negative electrodes called?

A

Positive electrode - anode

Negative electrode - cathode

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27
Q

Metal ions are positive or negative?

Non metal ions are positive or negative?

A

Metal ions are positive

Non metal ions are negative

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28
Q

Where do the positive and negative ions move to during electrolysis

A

Positive ions move to the cathode

Negative ions move to the anode

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29
Q

How does electrolysis work?

4 steps

A
  1. When you melt or dissolve an ionic compound in water it splits up into charged particles called ions
  2. Metal ions are positive
  3. Metal ions are attracted to the negative electrode (cathode) where they turn into metals
  4. Non-metal ions are attracted to the positive electrode (anode) where they form non-metals
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30
Q

Give the word and symbol equation of electrolysis for lead bromide

A

Lead is Pb2+ and Bromine is Br-
Pb2+ are attracted to the cathode so its
Pb2+ + 2e- —> Pb
Br- are attracted to the anode so its
2Br- - e- —> Br2

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31
Q

Why doesn’t aluminum shows it’s true reactivity?

A

Because as soon as its place in the air it reacts to from a tough oxide coat which protects and prevents it from reacting further

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32
Q

What is the ore called which aluminium is extracted from?

A

Bauxite

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33
Q

After mining and purifying bauxite, what are you left with?

A

Aluminium oxide (alumina) which is a white solid

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34
Q

What type of compound is aluminium oxide?

A

Ionic

35
Q

Do you have to melt aluminum oxide for it to conduct electricity?

A

Yes

36
Q

Does aluminium oxide have a high or low melting point?

Does it take lots or little amounts of electricity to split aluminum oxide?

It is a cheap or expensive process?

A

High melting point of around 2000 degrees Celsius

It takes lots of electricity to split it

It is an expensive process because it has a very high melting point?

37
Q

What can be done to reduce the cost of extracting aluminum from aluminum oxide?

A

Aluminium oxide can be mixed and dissolved with cryolite. Thus reduces the melting point to about 900 degrees and using molten cryolite as a solvent can reduce energy costs

38
Q

What are the aluminium ions attracted to during the process of extracting aluminum from aluminum oxide and give the symbol equation

A

Aluminium ions are attracted to the negative electrode and gain electrons to form aluminium metal
Al3+ + 3e- ——-> Al reduction

39
Q

What are the oxide ions attracted to during the process of extracting aluminum from aluminum oxide and give the symbol equation

A

Oxide ions are attracted to the positive electrode (anode) and lose electrons to form oxygen gas
202- - 4e- ——–> O2

40
Q

Why is the process of extracting aluminium expensive?

A

Because huge amounts of electricity is needed, that’s why all aluminum factories are nearly always built near power stations and lots of heat is needed. Also because the graphite anodes consist of carbon, oxygen forms at these anodes forming carbon dioxide This means they have to keep getting replaced

41
Q

What gets reduced and what gets oxidised during the electrolysis of aluminium oxide

A

Aluminum ions get reduced to form aluminum. This means that the negative electrode gains electrons

the oxide ions get oxidised to form oxygen. This means that that the positive electrode loses electrons

42
Q

Give 5 properties of aluminium

A 
Malleable
Ductile
Low density
Conducts electricity
Doesn't rust
43
Q

What is electroplating

A

This is when you coat your desired metal over another metal to protect against corrosion or improve its appearance

44
Q

What are the requirements for electroplating?

A

The negative electrode should be the object to be electroplated.

The positive electrode should be the metal that you want to coat the object with.

The electrolyte should be a solution of the coating metal, such as its metal nitrate or sulfate.

45
Q

Can copper metal be purified by electrolysis?

A

Yes

46
Q

What is the set up for the purification of copper

what is the anode made of, what is the cathode made of and what does the electrolyte contain

A

The anode is made from impure copper

The cathode is made from pure copper

The electrolyte contains copper ions from a solution such as copper sulphate solution

47
Q

During the electrolysis of copper (purification of copper). What happens

A

The anode dissolves so it gets smaller and the cathode gets bigger because it is coated with copper from the anode

48
Q

Give the ionic equation at the anode for the purification of copper

A

At the anode, Cu → Cu2+ + 2e– (oxidation)

49
Q

Give the ionic equation at the cathode for the purification of copper

A

At the cathode, Cu2+ + 2e– → Cu (reduction)

50
Q

What does the electrolysis of water split?

A

It splits hydrogen and oxygen

51
Q

What is the overall equation for the electrolysis of water?

A

2H2O —-> 2H2 + O2

52
Q

What happens at the cathode in the electrolysis of water. Give the equation as well

A

At the cathode a reduction reaction occurs. The positive hydrogen ions move to the cathode
4H+ + 4e- —-> 2H2

53
Q

What happens at the anode in the electrolysis of water. Give the equation as well

A

At the anode, an oxidation reaction occurs. The negative OH- ions move to the anode and lose electrons to form oxygen and water
4OH- —-> 2H2O + O2 + 4e-

54
Q

In the electrolysis of water, is there twice as much hydrogen gas produced?

A

Yes

55
Q

In the electrolysis of aqueous solution, what happens at the cathode

A

If a metal is more reactive than hydrogen, hydrogen will always form.
If a metal is less reactive than hydrogen, then that metal will form

56
Q

In the electrolysis of aqueous solution, what happens at the anode

A

Oxygen will always be produced unless the ionic compound contains halide ions (Cl-, Br-, I-)
If there are halide ions, the halogens will be produced instead

57
Q

In an aqueous solution of copper chloride

Where would the copper ions go to and where would the chloride ions go to

A

The copper ions (Cu+) go to the cathode where copper will be produced
The chloride ions (Cl-) will go to the anode where chlorine will be produced because it is a halide

58
Q

In an aqueous solution of sodium sulphate where would the sodium ions go and where would the sulphate ions go

A

Instead of the sodium, H+ ions will go to the cathode because it is sodium is more reactive than hydrogen
Instead of the sulphate ions, the OH- ions will go to the anode because sulphate ions are not halide

59
Q

In an aqueous solution of sodium chloride. Where would the Na+ ions go and where would the Cl- ions go

For this give the equations for each process and also give the manufacture of sodium hydroxide as well

A

The Na+ ions will go to the cathode to gain electrons to form sodium metal
Na+ + e- —-> Na Reduction

The Cl- ions will go to the anode to lose electrons to form chlorine gas
2Cl- - 2e- —-> Cl2 Oxidation

Sodium hydroxide

At the cathode, there is competition between the hydrogen ions and sodium ions and because the hydrogen ions gain electrons more easily and sodium is more reactive than hydrogen. Hydrogen is produced
to form hydrogen gas
2H+ + 2e- —-> H2 Redcution

At the anode, there is competition between the chloride and hydroxide ions. However, because chloride is a halide ion it wins and loses electrons to form chlorine gas
2Cl- - 2e- —-> Cl2 Oxidation

Because there are left over OH- ions and Na+ ions in the electrolyte, these react together to form sodium hydroxide.

60
Q

What are the uses of hydrogen

A

Rocket fuels
Manufacture of fertiliser
Make unsaturated oil to saturated fat

61
Q

What are the uses of Chlorine

A 
Bleach
Swimming pools to kill bacteria
Make hydrochloric acid 
PVC
Wellington boots
62
Q

What are the uses of Sodium Hydroxide

A

Soap
Oven cleaners
Paper manufacturers
Detergents

63
Q

What is the test to prove hydrogen gas is present

A

Get a lighted splint near gas and if hydrogen gas is present there is a pop

64
Q

What is the test to prove chlorine is present

A

Put damp litmus paper near gas and it will go white because chlorine is a bleach

65
Q

Where are transition metals found?

A

Between group 2 and group 3 of the periodic table

66
Q

Give 8 properties of metals

A 
High melting point
High boiling point
Hard
High density
Malleable
Ductile
Good conductors of heat and electricity
Lustrous (shiny and bright)
67
Q

When transition metals react, they ______ electrons to form ______ ions

A

When transition metals react, they lose electrons to form positive ions

68
Q

What are the 3 ions we need to know when talking about transition metals?

A

Fe3+
Fe2+
Cu2+

69
Q

What is the test we use to find the presence of Fe3+, Fe2+ and Cu2+ ions

A

We add a dilute sodium hydroxide solution

70
Q

What is the Cu2+ (transition metals) result from the test and what is the equation

A

It turns into a blue colour
Cu2+ is
Cu2+ (aq) + 2OH- (aq) —-> Cu(OH)2 (s)

71
Q

What is the Fe2+ (transition metals) result from the test and what is the equation

A

It turns into a pale green colour

Fe2+ is Fe2+ (aq) + 2OH- (aq) —-> Fe(OH)2 (s)

72
Q

What is the Fe3+ (transition metals) result from the test and what is the equation

A

It turns into a brown colour

Fe3+ is Fe3+ (aq) + 2OH- (aq) —-> Fe(OH)3 (s)

73
Q

What is an alloy?

A

A substance made of a mixture of 2 metals or at least a metal

74
Q

Why are alloys harder than metals?

A

Because alloys contain atoms of different sizes. These different sizes distort the regular arrangement of atoms which makes it more difficult for the layers to slide over each other.

75
Q

Give 3 examples of alloys

A

Steel - Iron (metal) and carbon (non-metal)
Brass - copper (metal) and zinc non-metal)
Bronze - Tin (metal) and copper (non-metal)

76
Q

The composition of alloys an be changed to produce alloys with desired _________

A

The composition of alloys an be changed to produce alloys with desired properties

77
Q

Properties and uses of steel x3 for each

A

very strong, good conductor of heat and electricity, can be magnetised
Can be used in saucepans, cutlery, build cars

78
Q

uses of aluminum

A

can be used in soda cans, manufacture of car bodies and window frames

79
Q

Properties and uses of copper

A

Very good conductor of heart and electricity, malleable and ductile, attractive colour and lustre
Can be used in wiring and motors, ornaments and jewellry

80
Q

Properties and uses of titanium

A

Hard, strong, low density, resistant to corrosion and high melting point
Can be used in air crafts, jewellery, sports equipment and medical implants

81
Q

low carbon steel properties:

A

Tough, ductile, malleable, strong and poor resistance to corrosion

82
Q

High carbon steel properties:

A

Hard, very strong, wear resistant and more brittle than low carbon steel

83
Q

Stainless steel properties:

A

Resistant to corrosion

84
Q

Steel is much _______ than iron and therefore more ______

A

Steel is much harder than iron and therefore more useful

Chemistry unit 2 GCSE (6 decks)

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