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AA IGCSE Chemistry > Metals and Metal Extraction > Flashcards

Metals and Metal Extraction Flashcards

1
Q

Why do metals have high boiling points?

A

because a metallic lattice is held together by strong forces of electrostatic attraction which require a lot of energy to overcome

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2
Q

Why are metals good electric conductors?

A

they have delocalised electrons which are free to move

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3
Q

Why are metals good thermal conductors?

A

they have delocalised electrons which move around the metal and transfer thermal energy to the ions

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4
Q

Why are metals malleable?

A

the ions are arranged in regular layers which can slide over each other and bend instead of break

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5
Q

Why are metals ductile?

A

layers slide over each other when pulled apart, forming a thin wire

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6
Q

What happens when a metal reacts with dilute acids?

A

they produce a salt and hydrogen

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7
Q

Write a general word equation for the reaction between metals and dilute acids.

A

metal + dilute acid -> salt + hydrogen

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8
Q

What happens when a metal reacts with water?

A

they form a metal hydroxide and hydrogen gas

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9
Q

Write a general word equation for the reaction between metals and water.

A

metal + water -> metal hydroxide + hydrogen gas

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10
Q

What happens when a metal reacts with oxygen?

A

they form metal oxides

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11
Q

Write a general word equation for the reaction between metals and oxygen.

A

metal + oxygen -> metal oxide

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12
Q

Name 3 uses of aluminium.

A
  1. manufacture of aircraft
  2. manufacture of overhead electrical cables
  3. food containers
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13
Q

What is one use of copper?

A

electrical wiring

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14
Q

Why is aluminium suitable for the manufacture of aircraft?

A

it has a low density

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15
Q

Why is aluminium suitable for the manufacture of overhead electrical cables?

A

it has a low density and is a good electrical conductor

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16
Q

Why is aluminium suitable for food containers?

A

it is resistant to corrosion

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17
Q

Why is copper suitable for electrical wiring?

A

it is a good electrical conductor and ductile

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18
Q

What is the order of the reactivity series, from most to least reactive?

A

potassium
sodium
calcium
magnesium
aluminium
carbon
zinc
iron
lead
hydrogen
copper
silver
gold

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19
Q

What are the three most reactive metals?

A

potassium, sodium and calcium

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20
Q

Describe the reaction between sodium and cold water.

A

floats
moves quickly
heat from reaction melts sodium

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21
Q

Describe the reaction between potassium and cold water.

A

floats
melts
catches fire- burns with a lilac coloured flame

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22
Q

Describe the reaction between calcium and cold water.

A

reacts quickly
water turns milky white

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23
Q

Describe the reaction between magnesium and steam.

A

reacts readily
forms magnesium oxide and hydrogen

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24
Q

Describe the reaction between zinc and dilute hydrochloric acid.

A

bubbles formed slowly

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25
Q

Which four metals react with water/steam?

A

potassium
sodium
calcium
magnesium

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26
Q

Describe the reaction between magnesium and dilute hydrochloric acid.

A

strong bubbles formed quickly

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27
Q

Describe the reaction between iron and dilute hydrochloric acid.

A

very slow reaction
must be powdered iron

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28
Q

Describe the reaction between copper and dilute hydrochloric acid.

A

none

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29
Q

Describe the reaction between silver and dilute hydrochloric acid.

A

none

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30
Q

Describe the reaction between gold and dilute hydrochloric acid.

A

none

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31
Q

In a displacement reaction, which metal will lose electrons?

A

the more reactive metal

32
Q

In a displacement reaction, which metal will gain electrons?

A

the less reactive metal

33
Q

Define oxidation

A

loss of electrons
increased oxidation number

34
Q

Define reduction

A

gain of electrons
decrease in oxidation number

35
Q

The more reactive a metal is, the more _____ it will lose its valence electrons.

A

easily

36
Q

State which metals have a higher tendency to form positive ions in a displacement reaction.

A

more reactive metals

37
Q

A ______ metal will displace a _______ metal.

A

more reactive
less reactive

38
Q

Is aluminium reactive? Why might we think otherwise?

A

aluminium IS reactive
oxide layer: surface atoms of aluminium react with oxygen in air to form an oxide layer, protecting the inner metal from corroding

39
Q

Define ‘metallic bonding’.

A

the electrostatic attraction between the positive ions in a giant metallic structure and the surrounding ‘sea’ of delocalised electrons

40
Q

Why are metals good electrical conductors?

A

there are many delocalised electrons that can flow

41
Q

Why are metals malleable?

A

because they are arranged in layers that slide over each other

42
Q

Define ‘alloy’.

A

a mixture of a metal with other elements

43
Q

What elements make up brass?

A

copper and zinc

44
Q

What elements make up stainless steel?

A

iron, and other elements such as chromium, nickel and carbon

45
Q

Why do people form alloys?

A

they can be harder, stronger and more useful than pure metals

46
Q

Why are alloys stronger/harder than pure metals?

A

different sized atoms in alloys prevent layers from sliding over each other

47
Q

What is a use of stainless steel?

A

cutlery

48
Q

Why is stainless steel used for cutlery?

A

hard
resistant to rusting

49
Q

What occurs in a redox reaction?

A

oxidation and reduction simultaneously
loss and gain of electrons

50
Q

What is the oxidation number of elements in their uncombined state? What are examples of this?

A

0
O2, Mg

51
Q

What is the sum of the oxidation numbers in a compound?

A

0

52
Q

What is an oxidising agent?

A

a substance that oxidises another substance, being reduced in the process

53
Q

What is a reducing agent?

A

a substance that reduces another substance, being oxidised in the process

54
Q

What are the conditions required for rusting?

A

oxygen and water

55
Q

Word equation for rusting

A

iron + water + oxygen → hydrated iron(III) oxide

56
Q

State 4 common barrier methods.

A

painting
greasing
coating with plastic
galvanising

57
Q

How do barrier methods prevent rusting?

A

they exclude oxygen and water so it does not get to the metal

58
Q

What substance increases the rate of rusting?

A

salt

59
Q

In which substances does rusting occur?

A

steel and iron

60
Q

Give an example of sacrificial protection.

A

galvanising

61
Q

What are barrier methods?

A

methods that prevent iron from getting in contact with oxygen and water, preventing rusting

62
Q

Why is it important to prevent rusting?

A

rusting weakens important structures such as ships, which is dangerous

63
Q

What is sacrificial protection?

A

covering iron/steel with a more reactive metal which slowly sacrifices itself for the iron/steel

64
Q

What is galvanising?

A

a specific form of sacrificial protection with zinc

65
Q

How can we extract more reactive metals from their ores?

A

electrolysis

66
Q

Which metals require electrolysis to be extracted from their ore?

A

metals above carbon in the reactivity series
potassium, sodium, calcium, magnesium, aluminium

67
Q

How can we extract somewhat reactive metals from their ores?

A

reduction, using carbon/coke/charcoal

68
Q

Which metals require reduction to be extracted from their ore?

A

zinc
iron
lead

69
Q

Which metals do not need to be extracted? Why?

A

copper, silver, gold, platinum
unreactive and occur native

70
Q

Describe the extraction of iron from hematite in the blast furnace.

A
  1. coke is burned, providing heat and producing carbon dioxide
  2. coke reacts with carbon dioxide to form carbon monoxide/carbon dioxide is reduced to carbon monoxide
  3. iron (III) oxide is reduced by carbon monoxide
  4. calcium carbonate is thermally decomposed to form calcium oxide and carbon dioxide
  5. calcium oxide and silicon dioxide react to form slag (CaSiO3)
71
Q

How is aluminium extracted?

A

electrolysis

72
Q

What is the main ore of aluminium?

A

bauxite

73
Q

Write the balanced symbol equation for the reduction of iron oxide in the blast furnace.

A

Fe2O3 + 3CO → 2Fe + 3CO2

74
Q

Write the balanced symbol equation for the formation of slag in the blast furnace.

A

CaO + SiO2 → CaSiO3

75
Q

Write the balanced symbol equation for the thermal decomposition of limestone in the blast furnace.

A

CaCO3 → CaO + CO2

76
Q

State the symbol equations for the extraction of iron from hematite

A

(a) C + O2 → CO2
(b) C + CO2 → 2CO
(c) Fe2O3 + 3CO → 2Fe + 3CO2
(d) CaCO3 → CaO + CO2
(e) CaO + SiO2 → CaSiO3

AA IGCSE Chemistry (18 decks)

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