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Chemistry > 2.3 Metals & Their Extraction > Flashcards

2.3 Metals & Their Extraction Flashcards

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1
Q

What are ores

A

Minerals found in the Earth’s crust
Contain metal compounds, from which metals can be extracted using chemical reactions

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2
Q

What does the method used to extract metals from their ores depend on?

A

The metal’s position in the reactivity series

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3
Q

Give 2 metals that are found native - what does this mean

A

Gold and silver - they don’t need to be extracted

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4
Q

What does the difficulty of extracting methods increase with

A

Reactivity

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5
Q

How are the most reactive metals extracted from their ores

A

Electrolysis

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6
Q

How are the metals in the middle of the reactivity series extracted from their ores

A

They are chemically reduced

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7
Q

How can the relative reactivity of metals be demonstrated

A

Displacement reactions

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8
Q

What happens in displacement reactions

A

A more reactive metal will displace a less reactive metal from a solution of one of its salts

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9
Q

Displacement reaction example

A

iron + copper(II)chloride –> iron chloride + copper
copper has been displaced by iron :( (now its alone)

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10
Q

What happens in a competition reaction

A

A more reactive metal removes oxygen from the oxide of a less reactive metal when a mixture of the 2 is heated

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11
Q

Example of a competition reaction

A

The thermit reaction

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12
Q

Thermit reaction equation

A

iron(III) oxide + aluminium –> iron + aluminium oxide

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13
Q

Thermit reaction used for?

A

USed to weld rails together on a railway track

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14
Q

What is oxidation

A

The gain of oxygen
The loss of electrons (OILRIG)

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15
Q

What is reduction

A

The loss of oxygen
The gain of electrons (OILRIG)

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16
Q

What are the raw materials used in the blast furnace (4)

A
  • iron ore - source of iron
  • coke - as a fuel & to produce carbon monoxide for the reduction
  • limestone - to remove impurities by forming slag
  • hot air - provides oxygen so coke can burn
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17
Q

What type of reaction is the production of iron in the blast furnace

A

Reduction

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18
Q

First step in the production of iron - blast furnace
Endothermic or exothermic

A

Oxygen from the hot air reacts with carbon (coke) to form carbon monoxide
Exothermic which heats the surface

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19
Q

Second step in the production of iron
What’s reduced?

A

Carbon dioxide then reacts with iron (III) oxide (from iron ore) to give iron
iron is reduced!

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20
Q

3rd step in the production of iron - blast furnace

A

Limestone deposits thermally to form calcium oxide

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21
Q

4th step in the production of iron - blast furnace

A

Calcium dioxide reacts with silicon dioxide (sand) to from slag; This is removed

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22
Q

Chemical equation of 1st step in production of iron

A

Oxygen from the hot air reacts with carbon (coke) to form carbon monoxide
2C + O2 –> 2CO

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23
Q

Chemical equation of 2nd step in production of iron

A

Carbon dioxide then reacts with iron (III) oxide (from iron ore) to give iron
iron is reduced!
Fe2O3 + 3CO –> 2Fe + 3CO2

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24
Q

Chemical equation of 3rd step in production of iron

A

Limestone deposits thermally to form calcium oxide
CaCO3 –> CaO + CO2

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25
Q

Chemical equation of 4th step in production of iron

A

Calcium dioxide reacts with silicon dioxide (sand) to from slag
CaO + SiO2 –> CaSiO3

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26
Q

What type of reaction is the production of iron in a blast furnace

A

Neutralisation as CaO is basic, silica is acid

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27
Q

Why is the production of iron in the blast furnace continuous

A

New raw materials are added and products remove all the time (due to the cost of getting the furnace hot enough)

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28
Q

Electrolysis defintion

A

The process of breaking down an ionic compound using electrical energy

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29
Q

Electrolyte definition

A

The liquid (so ions are free to move) which is broken down by an electrical charge

30
Q

Electrode defintion

A

Graphite rod which carries a current in and out of the electrolyte

31
Q

Cathode definition

A

Negative electrode
(PANIC)

32
Q

Anode definition

A

Positive electrode
(PANIC)

33
Q

Electrolysis of water- what is connected on the cathode and anode

A

Hydrogen gas collected on the cathode
Oxygen gas collected on the anode

34
Q

Electrolysis of water- equation for reaction at the cathode and anode

A

ANODE: 2OH- ➡️ O2 ➕ 2H+➕4e-

CATHODE: 2 H+ ➕ 2 e- ➡️ H2

35
Q

Why is the volume of H formed twice the volume of OH formed electrolysis of water

A

There are 2 H atoms for every O atom in a water molecule (H2O)

36
Q

What are the ions present in electrolysis of aqueous solutions (salt dissolved in water)

A

H+ ions and OH- ions as well as the ions from the dissolved salt

37
Q

When the dissolved salt includes metals lower than H in the reactivity series, what forms on the cathode

A

The metals (lower in reactivity series-less reactive)
e.g. COPPER Chloride
CATHODE Cu2+ ➕ 2e-➡️Cu
ANODE: 2Cl-➡️Cl2➕2e-

38
Q

When the dissolved salt includes ions from metals higher than H in the reactivity series, what forms at the cathode

A

Metals higher than H
e.g. sodium chloride solution
CATHODE: 2H+➕2e-➡️H
ANODE: 2Cl-➡️Cl2➕2e-

39
Q

What’s The industrial extraction of aluminium& from what

A

Electrolysis
Extraction of aluminium from aluminium dioxide

40
Q

What is the cathode in the electrolysis of aluminium

A

Carbon lining to the cell acts as the cathode

41
Q

What comes out of the electrolysis thingy aluminium electrolysis

A

Molten aluminium

42
Q

What ions are in the aluminium oxide electrolysis electrolyte

A

Al3+
O2-

43
Q

What can be found on the top of the aluminium electrolysis machine

A

Crust

44
Q

What is the aluminium oxide dissolved in at what temp and why

A

Molten cryolite
Temperature much lower than aluminium oxide melting point
Therefore saving energy

45
Q

Another word for aluminium oxide

A

Alumina

46
Q

Aluminium oxide electrolysis electrode equations

A

CATHODE: Al3+➕3e-➡️Al
ANODE: 2O2-➖4e-➡️O2
or 2O2-➡️O2➕4e-

47
Q

What does the oxygen formed in aluminium electrolysis do

A

Reacts with the carbon anodes, forming carbon dioxide gas and requiring anodes to be replaced frequently

48
Q

Factors impacting the location of aluminium plants

A

-near coast- to import raw materials
-away from built up areas
- town/city within commuting distance to accommodate the workforce
-good transport links to transport the product to buyers
- direct electricity supply

49
Q

Other considerations of aluminium plants

A
  • fuel and energy costs
  • Green house gas emission
  • recycling
50
Q

What is electroplating

A

A technique using electrolysis to coat one metal with another metal

51
Q

Electroplating uses

A

Gold plating- A cheap object can be coated with an expensive metal - jewellery
To modify other properties of the plated objects, e.g. resistant to corrosion - nickel plating

52
Q

How does purification of copper by electrolysis work? (Cathode, anode, electrolyte)

A

Anode = large block of impure copper
Cathode = thin piece of pure copper
Electrolyte = copper sulfate solution

53
Q

What happens at the cathode purification of copper

A

Copper is deposited by reduction
Cu2+(aq)➕2e-➡️Cu(s)

54
Q

What happens at the anode purification of copper

A

Copper atoms are oxidised and go into solution
Cu(s)➡️Cu2+(s)➕2e-

55
Q

Anions attracted to

A

Anode

56
Q

Cations attracted to

A

Cathode

57
Q

When the electrolysis Involves assault of a reactive metal which ions does the solution contains?

A

Positive ions of the reactive metal and positive hydrogen ions from the water as well as the negative ions of the salt and water

58
Q

Which Irons appear at the cathode when there is competition at the cathode between reactive metal and hydrogen

A

The more reactive irons remain in solution
More Reactive equals more stable
Less reactive gains electrons more easily

59
Q

Properties and uses of iron and steel

A

Strong and hard using magnets and iron cores for Transformers

60
Q

Uses and properties of aluminium

A

Strong, low-density resistant to corrosion
Uses: Overhead high-voltage power, cables, saucepans, cooking, non-toxic drink cans

61
Q

Copper uses and properties

A

Very good conductor of heat and electricity, malleable and ductile
Uses- Making alloys wires saucepan (heat conductors)

62
Q

Titanium properties and uses

A

Strong low density resistant to corrosion high melting point
Jet engine parts, spacecraft parts, Car parts, industrial plants

63
Q

Where are the transition metals found in the periodic table
What can they form?

A

Middle
More than one type of ion

64
Q

Colour of the compound or solution of Fe2+

A

Pale green

65
Q

Colour of the compound or solution of Fe3+

A

Brown

66
Q

Colour of the compound or solution of Cu2+

A

Blue

67
Q

How can we test for the presence of transition metals?

A

Using a solution of sodium hydroxide, precipitation reactions with OH- ions

68
Q

Cu2+ (aq)➕2OH-(aq)➡️Cu(OH)2 (s)
Colour of this precipitate (test for Cu2+ ions)

A

Blue precipitate

69
Q

Fe2+ (aq)➕2OH-(aq)➡️Fe(OH)2 (s)
Colour of this precipitate (test for Fe2+ ions)

A

Green precipitate

70
Q

Fe3+ (aq)➕2OH-(aq)➡️Fe(OH)3 (s)
Colour of this precipitate (test for Fe3+ ions)

A

Orange/brown precipitate

71
Q

What is an alloy?

A

A mixture of made by mixing molten metals

72
Q

How can alloys properties be modified?

A

its properties can be , modified by changing its composition

Chemistry (7 decks)

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