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

Topic 4 - Extracting Metals and Equilibrium Flashcards

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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

A

Iron oxide ore

25
Q

Malachite

A

Copper carbonate containing ore

26
Q

Disadvantages of electrolysis (2)

A
  • requires a lot of energy to melt metal
27
Q

Bioleaching (4)

A
  • Bacteria grown on low grade ore
28
Q

Metals extracted using bioleaching (4)

A

Nickel, cobalt, zinc, copper

29
Q

Phytoextraction

A

Growing plants that absorb metal compounds. The plants are then burnt to form ash from which metal is extracted.

30
Q

Advantages bioleaching (4)

A
  • conserves supplies high grade ore
31
Q

Disadvantages bioleaching (2)

A
  • very slow
32
Q

advantages of phytoextraction (4)

A
  • can extract metals from contaminated soils
33
Q

Disadvantages phytoextraction (2)

A
  • more expensive than mining
34
Q

Bauxite

A

A mineral used in making aluminum

35
Q

Why is aluminium more expensive than iron if it is more abundant?

A

Takes more energy in extraction process

36
Q

Why is aluminium oxide mixed with cryolite when extracting aluminium?

A

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
Q

Why must the anodes used in aluminium extraction be replaced?

A

Oxygen reacts with carbon anodes, forming CO2

38
Q

Steps to recycle a metal (3)

A

1) collect and transport used items to a recycling centre

39
Q

Advantages of recycling metals (3)

A

more economical - less energy is needed to recycle than produce a metal.

40
Q

Disadvantages of recycling (2)

A

labor intensive

41
Q

Life Cycle Assessment

A

Analysis of environmental impacts of products from the design stage through end-of-life.

42
Q

Stages of LCA (4)

A
  1. Obtaining raw materials
43
Q

Raw materials (2)

A
  • uses up limited resources eg crude oil
44
Q

Manufacture (2)

A
  • uses land for factories
45
Q

Use

A

Depends on how much maintenance a product needs, and how durable it is

46
Q

Disposal (2)

A

Using up land for landfill sites

47
Q

What chemical reactions are reversible?

A

All! (In principle)

48
Q

reversible reaction

A

a chemical reaction in which the products re-form the original reactants

49
Q

Decomposition of ammonium chloride

A

NH4CL(s) ⇌ NH3(g)+HCl(g)

50
Q

Dynamic equilibrium

A

Position attained in a reversible reaction when the net concentration of reactants and products stay the same

51
Q

What does ‘dynamic’ mean in dynamic equilibrium?

A

The forward and backwards reactions continue to occur at the same rate

52
Q

What prevents equilibrium being obtained?

A

If it does not take place in a closed system, and reactants or products can escape

53
Q

Haber process

A

N2(g) + 3H2(g)⇌2NH3(g)

54
Q

Haber process steps (5)

A
  1. Nitrogen (extracted from the air) and hydrogen (obtained from natural gas) are pumped through pipes.
55
Q

Molecules of gas are directly proportional to…

A

Gas pressure

56
Q

How does gas pressure change equilibrium

A

If pressure is increased, equilibrium position moves in the direction of fewer molecules of gas as the system attempts to decrease gas pressure

57
Q

How does concentration affect equilibrium?

A

If concentration of a reactant increases, the equilibrium position moves in the direction with less of the reactant

58
Q

How does temperature affect equilibrium

A

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
Q

In every reversible equation, one is endothermic and one is…

A

Exothermic

Edexcel GCSE Chemistry Higher (12 decks)

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