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Edexcel GCSE Chemistry Triple > TOPIC 4- EXTRACTING METALS AND EQUILIBRIA > Flashcards

TOPIC 4- EXTRACTING METALS AND EQUILIBRIA Flashcards

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1
Q

Micrometers in standard form

A

10^-6

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2
Q

Nanometers in standard form

A

10^-9

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3
Q

How big are nano particles

A

Range from 1-100nm and only contain a few hundred atoms

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4
Q

Why are nano particles used as catalysts?

A

Because they have large surface area in comparison to their volume

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5
Q

Example of a nanoparticle

A

Zinc oxide is used as sunscreen as it absorbs UV radiation while remaining transparent.

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6
Q

Advantages of nanoparticles

A

High surface area to volume ratio, catalytic

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7
Q

Disadvantages of nanoparticles

A

Long term effects are unknown, can enter our living cells, bad for environment

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8
Q

Metals reaction with acids tell you what about them

A

Their level of reactivity

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9
Q

Metal + acid&raquo_space; ?

A

Salt + hydrogen

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10
Q

How does the reactivity affect the speed of the reaction

A

The more reactive the metal, the quicker the rate of reaction

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11
Q

How do you confirm hydrogen is released?

A

Squeaky pop test

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12
Q

Mg + 2HCl» ?

A

MgCl2 + H2

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13
Q

How do you speed up the rate of reaction ?

A

Heat or catalyst

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14
Q

Which metals react with water

A

K, Na, Li, Ca

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15
Q

Metal + water&raquo_space; ?

A

Metal hydroxide + hydrogenk

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16
Q

Metal + steam»?

A

Metal oxide + hydrogen

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17
Q

Reactivity series in order from top

A

K, Na, Ca, Mg, Al, C, Zn, Fe, Sn, Pb, H, Cu, Ag, Au

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18
Q

What’s a redox reaction?

A

A reaction in which oxidation and reduction ocurr

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19
Q

How does the reactivity of a metal affect the temp in displacement

A

More reactive = more heat released

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20
Q

Define displacement

A

When a more reactive metal displaces a less reactive metal from its compound

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21
Q

Oxidation involving oxygen

A

When a substance gains oxygen

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22
Q

Reduction involving oxygen

A

When a substance loses oxygen

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23
Q

Oxidation with electrons

A

Loss of electrons

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24
Q

Reduction involving electrons

A

Gain of electrons

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25
Q

Half equation of each from: Mg + CuSO4> MgSO4 + Cu

A

Mg > Mg^2+ + 2e-

Cu^2+2e-> Cu

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26
Q

Oxidising agent

A

Accepts electrons and gets reduced

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27
Q

Reducing agent

A

Donates electrons and gets oxidised

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28
Q

Metal ore

A

A rock containing enough metal out of its compounds to make it economically viable to extract.

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29
Q

Ores vs the actual metal

A

They hav different properties

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30
Q

Mercury ore

A

Cinnabar

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31
Q

Aluminium ore

A

Bauxite

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32
Q

How does a metals reactivity affect its ease of extraction

A

The more reactive = the harder to extract

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33
Q

How do you extract metals below carbon in the reactivity series

A

Reduction with carbon

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34
Q

How do you extract metals above carbon in the reactivity series?

A

Electrolysis

35
Q

Metal oxide + carbon >?

A

metal + carbon dioxide

36
Q

Biological ways to extract low grade ores?

A

Bio leaching and phytomining

37
Q

What’s phytomining?

A

Planting crops in copper rich soil so that they absorb it through their roots. Plants are burnt to produce copper ash

38
Q

Advantages of phytomining

A

Carbon neutral

39
Q

Disadvantages of phytomining

A

Produces impure copper

40
Q

What’s bio leaching?

A

Bacteria that can absorb metal compounds to produce leachates that contain copper compounds.

41
Q

Disadvantages of bioleaching

A

V slow

42
Q

Why would (expensive) cryolite be mixed in with the compound before electrolysis.

A

To lower its mp

43
Q

Electrolysis

A

Breaking down of a substance using electricity

44
Q

Electrolyte

A

Molten or dissolved ionic compound

45
Q

Anode charge

A

Positive

46
Q

Cathode charge

A

Negative

47
Q

Flow of electrons

A

Anode to cathode

48
Q

What’s attracted to cathodes and what charge

A

Cations (positive)

49
Q

What’s attracted to anodes and what charge

A

Anions (negative)

50
Q

What happens when the cations reach the cathode?

A

They are reduced (gain electrons) and discharged.

51
Q

When anions move to the anode, what do they do?

A

They are oxidised (lose electrons) and so are discharged

52
Q

Ionic compound

A

Compound with a positive and negative ion formed in a lattice shape

53
Q

What electrons are used in electrolysis of molten ionic compounds?

A

Inert (unreactive) like lead for example

54
Q

What ions are included in electrolysis of aqueous solutions

A

H+, OH- and ionic compound

55
Q

What happens at the cathode in electrolysis of aqueous solutions?

A

If the metal is more reactive than hydrogen, hydrogen is produced. If the metal is less reactive than hydrogen, the metal is produced.

56
Q

What happens at the anode in electrolysis of aqueous solutions?

A

If a halide is present, the halide is produced. If there’s no halide present, oxygen and water is produced.

57
Q

What’s corrosion

A

The rusting of a metal. (The reaction of metal and oxygen)

58
Q

What do you need to corrode a metal?

A

Oxygen and water

59
Q

Metal + water + oxygen >?

A

Hydrated metal oxide

60
Q

How do you prevent corrosion

A

Coat it in a barrier (tarnish) or put a more reactive metal with it (metal coating)

61
Q

In purification if copper what’s the cathode made out of?

A

Pure copper

62
Q

In purification of copper, what’s the anode made out of?

A

Impure copper

63
Q

In purification of copper, what’s the electrolyte ?

A

Copper sulfate

64
Q

What’s the voltage directly proportionate to in purification of copper?

A

The mass of the cathode due to quicker donation and loss of electrons.

65
Q

What does the cathode do in purification of copper ?

A

It grows heavier due to reduction of copper ions leading to discharged atoms deposited on the cathode.

66
Q

What does the anode do during copper purification?

A

It grows lighter due to oxidisation of the impure copper molecules causing more copper to dissolve into the solution. The impurities are left as a slush at the bottom.

67
Q

Why do people keep pushing recycling of metals?

A

Because metal extraction is time consuming, expensive and harmful to the environment. Also forms of disposal are also very harmful to the environment.

68
Q

Advantages of recycling metals

A

Lower energy consumption/cost, saving of resources, less waste/pollutants and creation of jobs

69
Q

Disadvantages of recycling metals

A

Alloys are hard to recycle, transport cost/emissions, sorting, impurity of end product, and money cost to sort and collect

70
Q

What does the lifecycle assessment cover?

A

Extraction > manufacturing > use > disposal

71
Q

Landfill disadvantages

A

Takes up space, pollutes surroundings, doesn’t preserve materials

72
Q

Dynamic equilibrium

A

When the forwards and backwards reactions occur at the same rate, meaning concentrations of reactants and products won’t change

73
Q

What type of system do dynamic equilibriums take place in?

A

Closed

74
Q

Closed systems

A

A system in which no reactants/ products can escape.

75
Q

Equilibrium lying to the right

A

Concentration of products is greater than that of reactants.

76
Q

Equilibrium lying to the left

A

Concentration of reactants is greater than that of products

77
Q

Le Chatelier’s principle

A

If there’s a change in concentration, temperature or pressure in a reversible reaction, the equilibrium will move to counteract that change.

78
Q

What happens when you decrease the temperature of a reaction in equilibrium?

A

The equilibrium will shift to the exothermic direction to produce more heat.

79
Q

What happens when you increase the temp of a reaction in equilibrium?

A

The equation Librium shifts to the endothermic direction to take in heat and therefore decrease temp.

80
Q

What happens when you increase the pressure of a reaction in equilibrium?

A

The equilibrium will shift to side w fewer moles to reduce pressure

81
Q

What happens when you decrease the pressure of a reaction in equilibrium?

A

The equilibrium will shift to the side with more moles of gas to increase pressure.

82
Q

What happens when you increase concentration of reactants?

A

The equilibrium will shift to the right to produce more products.

83
Q

What happens when you increase concentration of products?

A

The equilibrium will shift to the left to produce more reactants.

Edexcel GCSE Chemistry Triple (14 decks)

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