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Edexcel GCSE Chemistry Higher > Topic 4 - Extracting Metals and Equilibrium > Flashcards

Topic 4 - Extracting Metals and Equilibrium Flashcards

(59 cards)

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1
Q

reactivity series of metals

A

Potassium, sodium, calcium, magnesium, aluminium, zinc, iron, tin, lead, copper, silver, gold, platinum

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2
Q

The more reactive a metal is… (2)

A

The more vigorous its reactions and the more easily it forms cations

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3
Q

Potassium and sodium reaction with water

A

Violent with cold water

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4
Q

Calcium, magnesium reaction with water

A

Slow with cold water, rapid with steam

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5
Q

Aluminium and zinc reaction with water

A

Usually no reaction

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6
Q

Iron reaction with water

A

Rusts slowly

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7
Q

Copper, silver and gold reaction with water

A

None

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8
Q

Potassium and sodium reaction with acid

A

Violent

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9
Q

Calcium, magnesium, aluminium reaction with acid

A

Rapid

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10
Q

Zinc and iron reaction with acid

A

Slow

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11
Q

Copper, silver and gold reaction with acid

A

None

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12
Q

Metal + water..

A

Metal hydroxide and hydrogen

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13
Q

Metal + steam…

A

Metal oxide and hydrogen

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14
Q

Metal and acid..

A

Salt and hydrogen

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15
Q

Which metals dont react with acid?

A

Those below hydrogen in the reactivity series

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16
Q

Metal displacement reactions

A

A more reactive metal can displace a less reactive metal from a compound, are REDOX reactions

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17
Q

Ore definition

A

A rock that contains enough of a metal or metal compound to make extracting the metal worthwhile

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18
Q

Low grade ore vs high grade ore

A

Low - small percentage of metal or compound

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19
Q

Extraction with carbon (3)

A

Only works with metals less reactive than carbon

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20
Q

What does it mean if metals are found in their native state?

A

Very unreactive elements (gold, silver, platinum) found as uncombined elemnts

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21
Q

Metals electrolysed to purify (5)

A

Potassium, sodium, calcium, magnesium, aluminium

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22
Q

Metal oxides heated with carbon to purify (3)

A

Zinc, iron, copper

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23
Q

Native state elements (2)

A

Silver, gold

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24
Q

Haematite

Study These Flashcards
A

Iron oxide ore

25
Malachite
Copper carbonate containing ore
26
Disadvantages of electrolysis (2)
- requires a lot of energy to melt metal
27
Bioleaching (4)
- Bacteria grown on low grade ore
28
Metals extracted using bioleaching (4)
Nickel, cobalt, zinc, copper
29
Phytoextraction
Growing plants that absorb metal compounds. The plants are then burnt to form ash from which metal is extracted.
30
Advantages bioleaching (4)
- conserves supplies high grade ore
31
Disadvantages bioleaching (2)
- very slow
32
advantages of phytoextraction (4)
- can extract metals from contaminated soils
33
Disadvantages phytoextraction (2)
- more expensive than mining
34
Bauxite
A mineral used in making aluminum
35
Why is aluminium more expensive than iron if it is more abundant?
Takes more energy in extraction process
36
Why is aluminium oxide mixed with cryolite when extracting aluminium?
To lower the melting point of the aluminium oxide, so less energy needed to melt it (aluminium oxide insoluble in water so can't be aqueous)
37
Why must the anodes used in aluminium extraction be replaced?
Oxygen reacts with carbon anodes, forming CO2
38
Steps to recycle a metal (3)
1) collect and transport used items to a recycling centre
39
Advantages of recycling metals (3)
more economical - less energy is needed to recycle than produce a metal.
40
Disadvantages of recycling (2)
labor intensive
41
Life Cycle Assessment
Analysis of environmental impacts of products from the design stage through end-of-life.
42
Stages of LCA (4)
1. Obtaining raw materials
43
Raw materials (2)
- uses up limited resources eg crude oil
44
Manufacture (2)
- uses land for factories
45
Use
Depends on how much maintenance a product needs, and how durable it is
46
Disposal (2)
Using up land for landfill sites
47
What chemical reactions are reversible?
All! (In principle)
48
reversible reaction
a chemical reaction in which the products re-form the original reactants
49
Decomposition of ammonium chloride
NH4CL(s) ⇌ NH3(g)+HCl(g)
50
Dynamic equilibrium
Position attained in a reversible reaction when the net concentration of reactants and products stay the same
51
What does 'dynamic' mean in dynamic equilibrium?
The forward and backwards reactions continue to occur at the same rate
52
What prevents equilibrium being obtained?
If it does not take place in a closed system, and reactants or products can escape
53
Haber process
N2(g) + 3H2(g)⇌2NH3(g)
54
Haber process steps (5)
1. Nitrogen (extracted from the air) and hydrogen (obtained from natural gas) are pumped through pipes.
55
Molecules of gas are directly proportional to...
Gas pressure
56
How does gas pressure change equilibrium
If pressure is increased, equilibrium position moves in the direction of fewer molecules of gas as the system attempts to decrease gas pressure
57
How does concentration affect equilibrium?
If concentration of a reactant increases, the equilibrium position moves in the direction with less of the reactant
58
How does temperature affect equilibrium
If the temperature is increased, the equilibrium moves in the direction of the endothermic process as the system uses up the extra heat energy
59
In every reversible equation, one is endothermic and one is...
Exothermic

Edexcel GCSE Chemistry Higher (12 decks)

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