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iGCSE Chemistry > 3.5 Metals > Flashcards

3.5 Metals Flashcards

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1
Q

What is the structure of metallic bonding?

A
  • lattice of positive metal ions
  • sea of delocalised electrons
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2
Q

Define metallic bonding

A

electrostatic attraction between positive metal ions and negative delocalised electrons

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3
Q

Why do metals have high melting points?

A
  • metallic bonding is very strong
  • lots of energy needed to break
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4
Q

How are metals able to conduct electricity?

A
  • delocalized electrons are free to move
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5
Q

Why are metals so malleable?

A
  • layers of metal ions that can slide over each other
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6
Q

What are the properties of metals?

A

high melting points
malleable
conduct electricity

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7
Q

What is thermal decomposition?

A

heat energy used to break down a substance

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8
Q

What is metal carbonate decomposition?

A

when metal carbonate thermally decomposes to form
- metal oxide
- carbon dioxide

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9
Q

What does metal carbonate decomposition form?

A

metal oxide
carbon dioxide

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10
Q

What is downward delivery?

A

carbon dioxide sinks to the bottom of tube and remains there bc it is denser than air

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11
Q

What are some examples of low reactive metals?

A

Au
Ag
Cu
also H is here

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12
Q

What are Au, Ag and Cu?

A

low reactive metals

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13
Q

What are some examples of medium reactive metals?

A

Pb
Fe
Zn
also C is here

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14
Q

What are Pb, Fe and Zn?

A

medium reactive metals

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15
Q

What are some examples of high reactive metals?

A

C is also here
Al
Mg
Ca
Li
Na
K

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16
Q

How do I remember the metal reactivity series?

A

Au!
Agnes
Cut
Herself
Phoebe
Fell
Zamn!
Careful!
Alright
My guys
CaLifornia
Nah
K

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17
Q

What happens in metal + water reactions?

A

metal + water -> metal hydroxide + hydrogen

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18
Q

What is formed in metal + water reactions?

A

metal hydroxide + hydrogen

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19
Q

What are the observations of metal + water reactions?

A

effervescence
solid disappears

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20
Q

Why does effervescence occur in metal + water reactions?

A

hydrogen gas produced

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21
Q

Why does the solid disappear in metal + water reactions?

A

used up in the reaction

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22
Q

What forms when the metal + water reaction has happened?

A

an alkali
hydroxide is donated to water

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23
Q

What is different when Group 1 metals react with water?

A

very violent

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24
Q

What happens when Lithium reacts with water? (4)

A

solid floats
effervescence
solid moves
solid disappears

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25
Q

Why does the solid float when group 1 metals react with water?

A

less dense than water

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26
Q

Why does the solid move when group 1 metals react with water?

A

effervescence propels it around the surface of the water

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27
Q

What happens when Sodium reacts with water? (5)

A

solid floats
effervescence
solid moves
solid disappears
sodium melts

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28
Q

What happens when Potassium reacts with water? (6)

A

solid floats
effervescence
solid moves
solid disappears
potassium melts
lilac flame

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29
Q

What happens to group 1 metals as you go down the group?

A

increase in reactivity

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30
Q

Why do group 1 metals increase in reactivity as you go down the group?

A
  • atoms get bigger
  • have more shells
  • outer-electron is further away
  • attraction is weaker
  • less energy needed to break attraction
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31
Q

What does a metal + steam reaction produce?

A

metal + steam -> metal oxide + hydrogen

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32
Q

How is metal reacting with water different than reacting with steam?

A

hot steam has more energy
both bonds in water molecule break
so metal oxide not hydroxide

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33
Q

What does a metal + acid produce?

A

metal + acid -> salt + hydrogen

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34
Q

What is a salt?

A

compound formed when H is displaced from an acid

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35
Q

What are the observations of a metal + acid reaction?

A

metal disappears
effervescence

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36
Q

Why does the metal disappear in a metal + acid reaction?

A

used up in reaction

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37
Q

Why does effervescence occur in a metal + acid reaction?

A

hydrogen gas is produced

38
Q

What is the test for hydrogen?

A

lit splint -> squeaky pop
combustion of hydrogen causes test tube to resonate

39
Q

The more reactive a metal is…

A

the faster it will react with an acid

40
Q

Why cannot reactions between acids and low reactivity metals happen?

A

less reactive than hydrogen so cannot displace it to form the salt

41
Q

Why cannot reactions between acids and high reactivity metals happen?

A

reaction with acids is too violent

42
Q

How do displacement reactions between metals work?

A

more reactive metals displace less reactive metals

43
Q

What observations should I consider in a metal displacement?

A

solid colour change
solution colour change

44
Q

What are ores?

A

metals found in earth’s crust naturally in compound with oxygen or sulphur

45
Q

What are natives?

A

metals that are not naturally in compound with oxygen or sulphur because they are less reactive then S or O

46
Q

Give examples of metals that could form ores

A

C
H
Pb
Fe
Zn
C
Al
Mg
Ca
Li
Na
K

47
Q

Give examples of metals that form natives

A

Au
Ag

48
Q

Why do native metals not need to be chemically extracted?

A

they are so unreactive
they exist on their own

49
Q

How are ores chemically extracted?

A

depending on their reactivity

50
Q

How are high reactive metal ores chemically extracted?

A

using electricity

51
Q

How are medium reactive metal ores and copper ore chemically extracted?

A

carbon extraction
metal can be displaced by heating with carbon

52
Q

Why are high reactive metal ores chemically extracted using electricity?

A

more reactive than carbon

53
Q

Why are medium reactive metal ores and copper ore chemically extracted by carbon extraction?

A

less reactive than carbon

54
Q

Define reduction

A

loss of oxygen

55
Q

Define oxidation

A

gain of oxygen

56
Q

Define reducing agent

A

takes oxygen away

57
Q

Define oxidising agent

A

gives oxygen

58
Q

Define redox

A

reduction and oxidation in same reaction

59
Q

What is the chemical name for rust?

A

hydrated iron(III) oxide

60
Q

What are the properties of iron before rust?

A

shiny
grey
malleable

61
Q

What are the properties of iron after rust?

A

dull
brown
brittle

62
Q

What substances does rusting require?

A

oxygen
water

63
Q

How does rusting work?

A

iron is oxidized by o2
iron is hydrated by water

64
Q

How can rusting be prevented?

A

barriers
galvanisation
sacrificial protection

65
Q

How do barriers prevent rusting?

A

paint, plastic, oil, grease
only works if coating is intact
as soon as it breaks then rusting happens

66
Q

What is paint and plastic used for in barriers for preventing rusting?

A

stationary objects
buckets

67
Q

What is oil and grease used for in barriers for preventing rusting?

A

moving parts
bike chains

68
Q

How does sacrificial protection prevent rusting?

A

high reactive metal sacrifices
displaces iron from rust as soon as rust form

69
Q

What is the disadvantage to using sacrificial protection to prevent rusting?

A

high reactive metal must be replaced often

70
Q

What is the disadvantage to using barriers to prevent rusting?

A

only works if coating is intact
as soon as it breaks then rusting happens

71
Q

How does galvanisation prevent rusting?

A

coating iron with zinc
coating prevents contact
zinc displaces iron
sacrificial and barrier!

72
Q

What are common alloys?

A

steel
bronze
brass

73
Q

What is steel made of?

A

iron + carbon

74
Q

What is bronze made of?

A

copper + zinc

75
Q

What is brass made of?

A

copper + tin

76
Q

Why are alloys ‘harder’ than pure metals?

A

different sized atoms
prevents sliding of metal ions

77
Q

Why are alloys not malleable?

A

different sized atoms
prevents sliding of metal ions

78
Q

What is iron used for?

A

making steel

79
Q

Why is iron useful?

A

steel is more useful than iron

80
Q

What is low carbon steel made of?

A

Fe
0.1 % C

81
Q

What is low carbon steel used for?

A

ships
cars
bridges

82
Q

Why is low carbon steel useful?

A

strong
can be hammered into shape

83
Q

What is high carbon steel made of?

A

Fe
1 % C

84
Q

What is high carbon steel used for?

A

tools
knives
screwdrivers

85
Q

Why is high carbon steel useful?

A

less malleable
stiff

86
Q

What is stainless steel made of?

A

Fe
1 % C
10 % Cr

87
Q

What is stainless steel used for?

A

cutlery
cooking utensils
kitchen sinks

88
Q

Why is stainless steel useful?

A

Cr forms oxide layer
resists corrosion
stays shiny and clean

89
Q

What is copper used for?

A

wires
cooking pans
water pipes

90
Q

Why is copper useful?

A

conducts heat and electricity
unreactive
malleable

91
Q

What is aluminium used for?

A

aircraft bodies
power cables

92
Q

Why is aluminium useful?

A

low density
high strength
conductor

iGCSE Chemistry (17 decks)

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