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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
Why does the solid float when group 1 metals react with water?
less dense than water
26
Why does the solid move when group 1 metals react with water?
effervescence propels it around the surface of the water
27
What happens when Sodium reacts with water? (5)
solid floats effervescence solid moves solid disappears sodium melts
28
What happens when Potassium reacts with water? (6)
solid floats effervescence solid moves solid disappears potassium melts lilac flame
29
What happens to group 1 metals as you go down the group?
increase in reactivity
30
Why do group 1 metals increase in reactivity as you go down the group?
- atoms get bigger - have more shells - outer-electron is further away - attraction is weaker - less energy needed to break attraction
31
What does a metal + steam reaction produce?
metal + steam -> metal oxide + hydrogen
32
How is metal reacting with water different than reacting with steam?
hot steam has more energy both bonds in water molecule break so metal oxide not hydroxide
33
What does a metal + acid produce?
metal + acid -> salt + hydrogen
34
What is a salt?
compound formed when H is displaced from an acid
35
What are the observations of a metal + acid reaction?
metal disappears effervescence
36
Why does the metal disappear in a metal + acid reaction?
used up in reaction
37
Why does effervescence occur in a metal + acid reaction?
hydrogen gas is produced
38
What is the test for hydrogen?
lit splint -> squeaky pop combustion of hydrogen causes test tube to resonate
39
The more reactive a metal is...
the faster it will react with an acid
40
Why cannot reactions between acids and low reactivity metals happen?
less reactive than hydrogen so cannot displace it to form the salt
41
Why cannot reactions between acids and high reactivity metals happen?
reaction with acids is too violent
42
How do displacement reactions between metals work?
more reactive metals displace less reactive metals
43
What observations should I consider in a metal displacement?
solid colour change solution colour change
44
What are ores?
metals found in earth's crust naturally in compound with oxygen or sulphur
45
What are natives?
metals that are not naturally in compound with oxygen or sulphur because they are less reactive then S or O
46
Give examples of metals that could form ores
C H Pb Fe Zn C Al Mg Ca Li Na K
47
Give examples of metals that form natives
Au Ag
48
Why do native metals not need to be chemically extracted?
they are so unreactive they exist on their own
49
How are ores chemically extracted?
depending on their reactivity
50
How are high reactive metal ores chemically extracted?
using electricity
51
How are medium reactive metal ores and copper ore chemically extracted?
carbon extraction metal can be displaced by heating with carbon
52
Why are high reactive metal ores chemically extracted using electricity?
more reactive than carbon
53
Why are medium reactive metal ores and copper ore chemically extracted by carbon extraction?
less reactive than carbon
54
Define reduction
loss of oxygen
55
Define oxidation
gain of oxygen
56
Define reducing agent
takes oxygen away
57
Define oxidising agent
gives oxygen
58
Define redox
reduction and oxidation in same reaction
59
What is the chemical name for rust?
hydrated iron(III) oxide
60
What are the properties of iron before rust?
shiny grey malleable
61
What are the properties of iron after rust?
dull brown brittle
62
What substances does rusting require?
oxygen water
63
How does rusting work?
iron is oxidized by o2 iron is hydrated by water
64
How can rusting be prevented?
barriers galvanisation sacrificial protection
65
How do barriers prevent rusting?
paint, plastic, oil, grease only works if coating is intact as soon as it breaks then rusting happens
66
What is paint and plastic used for in barriers for preventing rusting?
stationary objects buckets
67
What is oil and grease used for in barriers for preventing rusting?
moving parts bike chains
68
How does sacrificial protection prevent rusting?
high reactive metal *sacrifices* displaces iron from rust as soon as rust form
69
What is the disadvantage to using sacrificial protection to prevent rusting?
high reactive metal must be replaced often
70
What is the disadvantage to using barriers to prevent rusting?
only works if coating is intact as soon as it breaks then rusting happens
71
How does galvanisation prevent rusting?
coating iron with zinc coating prevents contact zinc displaces iron sacrificial and barrier!
72
What are common alloys?
steel bronze brass
73
What is steel made of?
iron + carbon
74
What is bronze made of?
copper + zinc
75
What is brass made of?
copper + tin
76
Why are alloys 'harder' than pure metals?
different sized atoms prevents sliding of metal ions
77
Why are alloys not malleable?
different sized atoms prevents sliding of metal ions
78
What is iron used for?
making steel
79
Why is iron useful?
steel is more useful than iron
80
What is low carbon steel made of?
Fe 0.1 % C
81
What is low carbon steel used for?
ships cars bridges
82
Why is low carbon steel useful?
strong can be hammered into shape
83
What is high carbon steel made of?
Fe 1 % C
84
What is high carbon steel used for?
tools knives screwdrivers
85
Why is high carbon steel useful?
less malleable stiff
86
What is stainless steel made of?
Fe 1 % C 10 % Cr
87
What is stainless steel used for?
cutlery cooking utensils kitchen sinks
88
Why is stainless steel useful?
Cr forms oxide layer resists corrosion stays shiny and clean
89
What is copper used for?
wires cooking pans water pipes
90
Why is copper useful?
conducts heat and electricity unreactive malleable
91
What is aluminium used for?
aircraft bodies power cables
92
Why is aluminium useful?
low density high strength conductor

iGCSE Chemistry (17 decks)

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