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Chemistry > 2.3 Metals & Their Extraction > Flashcards

2.3 Metals & Their Extraction Flashcards

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
Chemical equation of 4th step in production of iron
Calcium dioxide reacts with silicon dioxide (sand) to from slag CaO + SiO2 --> CaSiO3
26
What type of reaction is the production of iron in a blast furnace
Neutralisation as CaO is basic, silica is acid
27
Why is the production of iron in the blast furnace continuous
New raw materials are added and products remove all the time (due to the cost of getting the furnace hot enough)
28
Electrolysis defintion
The process of breaking down an ionic compound using electrical energy
29
Electrolyte definition
The liquid (so ions are free to move) which is broken down by an electrical charge
30
Electrode defintion
Graphite rod which carries a current in and out of the electrolyte
31
Cathode definition
Negative electrode (PANIC)
32
Anode definition
Positive electrode (PANIC)
33
Electrolysis of water- what is connected on the cathode and anode
Hydrogen gas collected on the cathode Oxygen gas collected on the anode
34
Electrolysis of water- equation for reaction at the cathode and anode
ANODE: 2OH- ➡️ O2 ➕ 2H+➕4e- CATHODE: 2 H+ ➕ 2 e- ➡️ H2
35
Why is the volume of H formed twice the volume of OH formed electrolysis of water
There are 2 H atoms for every O atom in a water molecule (H2O)
36
What are the ions present in electrolysis of aqueous solutions (salt dissolved in water)
H+ ions and OH- ions as well as the ions from the dissolved salt
37
When the dissolved salt includes metals lower than H in the reactivity series, what forms on the cathode
The metals (lower in reactivity series-less reactive) e.g. COPPER Chloride CATHODE Cu2+ ➕ 2e-➡️Cu ANODE: 2Cl-➡️Cl2➕2e-
38
When the dissolved salt includes ions from metals higher than H in the reactivity series, what forms at the cathode
Metals higher than H e.g. sodium chloride solution CATHODE: 2H+➕2e-➡️H ANODE: 2Cl-➡️Cl2➕2e-
39
What’s The industrial extraction of aluminium& from what
Electrolysis Extraction of aluminium from aluminium dioxide
40
What is the cathode in the electrolysis of aluminium
Carbon lining to the cell acts as the cathode
41
What comes out of the electrolysis thingy aluminium electrolysis
Molten aluminium
42
What ions are in the aluminium oxide electrolysis electrolyte
Al3+ O2-
43
What can be found on the top of the aluminium electrolysis machine
Crust
44
What is the aluminium oxide dissolved in at what temp and why
Molten cryolite Temperature much lower than aluminium oxide melting point Therefore saving energy
45
Another word for aluminium oxide
Alumina
46
Aluminium oxide electrolysis electrode equations
CATHODE: Al3+➕3e-➡️Al ANODE: 2O2-➖4e-➡️O2 or 2O2-➡️O2➕4e-
47
What does the oxygen formed in aluminium electrolysis do
Reacts with the carbon anodes, forming carbon dioxide gas and requiring anodes to be replaced frequently
48
Factors impacting the location of aluminium plants
-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
Other considerations of aluminium plants
- fuel and energy costs - Green house gas emission - recycling
50
What is electroplating
A technique using electrolysis to coat one metal with another metal
51
Electroplating uses
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
How does purification of copper by electrolysis work? (Cathode, anode, electrolyte)
Anode = large block of impure copper Cathode = thin piece of pure copper Electrolyte = copper sulfate solution
53
What happens at the cathode purification of copper
Copper is deposited by reduction Cu2+(aq)➕2e-➡️Cu(s)
54
What happens at the anode purification of copper
Copper atoms are oxidised and go into solution Cu(s)➡️Cu2+(s)➕2e-
55
Anions attracted to
Anode
56
Cations attracted to
Cathode
57
When the electrolysis Involves assault of a reactive metal which ions does the solution contains?
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
Which Irons appear at the cathode when there is competition at the cathode between reactive metal and hydrogen
The more reactive irons remain in solution More Reactive equals more stable Less reactive gains electrons more easily
59
Properties and uses of iron and steel
Strong and hard using magnets and iron cores for Transformers
60
Uses and properties of aluminium
Strong, low-density resistant to corrosion Uses: Overhead high-voltage power, cables, saucepans, cooking, non-toxic drink cans
61
Copper uses and properties
Very good conductor of heat and electricity, malleable and ductile Uses- Making alloys wires saucepan (heat conductors)
62
Titanium properties and uses
Strong low density resistant to corrosion high melting point Jet engine parts, spacecraft parts, Car parts, industrial plants
63
Where are the transition metals found in the periodic table What can they form?
Middle More than one type of ion
64
Colour of the compound or solution of Fe2+
Pale green
65
Colour of the compound or solution of Fe3+
Brown
66
Colour of the compound or solution of Cu2+
Blue
67
How can we test for the presence of transition metals?
Using a solution of sodium hydroxide, precipitation reactions with OH- ions
68
Cu2+ (aq)➕2OH-(aq)➡️Cu(OH)2 (s) Colour of this precipitate (test for Cu2+ ions)
Blue precipitate
69
Fe2+ (aq)➕2OH-(aq)➡️Fe(OH)2 (s) Colour of this precipitate (test for Fe2+ ions)
Green precipitate
70
Fe3+ (aq)➕2OH-(aq)➡️Fe(OH)3 (s) Colour of this precipitate (test for Fe3+ ions)
Orange/brown precipitate
71
What is an alloy?
A mixture of made by mixing molten metals
72
How can alloys properties be modified?
its properties can be , modified by changing its composition

Chemistry (7 decks)

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