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Metals & the reactivity series Flashcards

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1
Q

what is the order of the reactivity series?

A
  • Potassium (K)
  • Sodium (Na)
  • Lithium (Li)
  • Calcium (Ca)
  • Magnesium (Mg)
  • Aluminium (Al)
  • Carbon (C)
  • Zinc (Zn)
  • Iron (Fe)
  • Copper (Cu)
  • Silver (Ag)
  • Gold (Au)
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2
Q

How can we gauge the position of metals in the reactivity series based on their reactions with water?

A
  • the most reactive metals will react very strongly even with water, so the metals higher in the reactivity series will have the strongest reactions
  • the least reactive metals will have the weakest or even no reactions with water, so the metals lower in the reactivity series will have these sorts of reactions
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3
Q

what is the word equation for the reaction of metals with water?

A

metal + water => metal hydroxide + hydrogen

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4
Q

How can we gauge the position of metals in the reactivity series based on their reactions with dilute hydrochloric or sulfuric acids?

A
  • metals that are highest in the reactivity series would have already have had a strong reaction with water ∴ we know that its reaction with acid would be waaaay stronger and EXPLOSIVELY EXOTHERMIC
  • metals that are lowest in the reactivity series would have little/no reaction with acid
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5
Q

what is the word equation for the reaction of a metal with acid?

A

metal + acid => metal salt + hydrogen

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6
Q

why doesn’t a reaction occur with aluminium and acid unless the acid is concentrated or heated?

A
  • aluminium has a protective oxide layer on its surface (caused by reacting with oxygen in the air) that prevents the aluminium beneath from reacting with the acid
  • concentrated or heated acid breaks down this oxide layer, allowing the aluminium to react with the acid
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7
Q

PRACTICAL1 - reaction of magnesium with hydrochloric acid and sulfuric acid

A

Mg (s) + H2SO4 (aq) => MgSO4 (aq) + H2 (g)

Mg (s) + HCl (aq) => MgCl2 (aq) + H2 (g)

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8
Q

observations for the reaction of magnesium with both hydrochloric and sulfuric acid

A
  • metal floats
  • metal disappears
  • effervescence
  • heat is given off
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9
Q

PRACTICAL2 - reaction of zinc with hydrochloric acid and sulfuric acid

A

Zn (s) + H2SO4 (aq) => ZnSO4 (aq) + H2 (g)

Zn (s) + HCl (aq) => ZnCl2 (aq) + H2 (g)

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10
Q

observations for the reaction of zinc with both hydrochloric and sulfuric acid

A

rapid fizzing/effervescence

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11
Q

PRACTICAL3 - reaction of iron with hydrochloric acid and sulfuric acid

A

Fe (s) + H2SO4 (aq) => FeSO4 (aq) + H2 (g)

Fe (s) + HCl (aq) => FeCl2 (aq) + H2 (g)

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12
Q

observations for the reaction of iron with both hydrochloric and sulfuric acid

A

a few small bubbles are formed

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13
Q

what do the reactions of Mg, Zn and Fe with acid tell us about their relative reactivity?

A
  • Mg had most vigorous reaction ∴ is the most reactive
  • Zn’s reaction was less strong than the Mg, but stronger than the Fe ∴ is in the middle
  • Fe had the weakest reaction ∴ is the least reactive of the three metals
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14
Q

when do displacement reactions occur?

A

a displacement reaction occurs when a metal is reactive enough to replace another metal out of its compound

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15
Q

how can we tell the reactivity of a metal based on a displacement reaction of a metal with a metal oxide?

A

The more reactive metal (whether in a compound or as an element):
- stays in the compound if already combined and the other metal is less reactive
- displaces a less reactive metal from its oxide or salt solution if it’s the free element
- the metal that does the displacing is more reactive; the one displaced or unable to displace is less reactive
- this shows that a more reactive metal donates electrons more readily, reducing the less reactive metal’s ions or oxide

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16
Q

general equation for the displacement reaction of a metal and a metal oxide

A

More reactive metal + Metal oxide → More reactive metal oxide + Less reactive metal

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17
Q

how can we tell the reactivity of a metal based on a displacement reaction of a metal with aqueous solutions of metal salts?

A

The more reactive metal (whether in a compound or as an element):
- stays in the salt solution as ions if already dissolved and the other metal is less reactive
- displaces a less reactive metal from its aqueous salt solution if it’s the free element
- the metal that does the displacing is more reactive; the one displaced or that doesn’t displace is less reactive
- this shows that more reactive metals give up electrons more easily, reducing the less reactive metal ions to solid metal

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18
Q

general equation for the displacement reaction of a metal and an aqueous metal salt solution

A

More reactive metal + Metal salt solution → Metal salt of reactive metal + Less reactive metal

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19
Q

what is a reactive metal?

A

a metal which is more stable (i.e has a full outer shell) as an ion than as an atom ∴ reacts with other atoms to become an ion

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20
Q

what is an unreactive metal?

A

a metal which is more stable (i.e has a full outer shell) as an atom than as an ion ∴ doesn’t need to react with other atoms

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21
Q

name the things that must be present in order for rusting to occur

A

water and oxygen

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22
Q

what is the chemical name and formula for rust?

A
  • name = hydrated iron (III) oxide
  • formula = Fe2O3.XH2O
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23
Q

word equation for rusting

A

iron + oxygen + water => hydrated iron (III) oxide

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24
Q

balanced symbol equation for rust formation

A

4Fe (s) + 3O2 (g) == H2O==> 2Fe2O3 (s)

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25
ionic equation for rusting
Fe3+ => Fe + 3e-
26
name the 3 rust prevention methods
- barriers - galvanising - sacrificial protection
27
name some examples of the barrier method
- painting - oiling/greasing - plastic coating
28
explain how the barrier method prevents rust formation
creates a physical barrier over the iron to prevent any contact with the oxygen and water (vapour) in the air, preventing the formation of rust
29
advantages of the barrier method
- plastic coating and painting are cheap, effective and hard wearing - oiling is flexible and easily covers metal moving parts - tin coating is long-lasting
30
disadvantages of the barrier method
- plastic coating may be bulky - paint is inflexible and chips easily - oiling wears off quickly - rusting can occur when a tin coating is chipped
31
what is galvanising?
when an iron structure is dipped into molten zinc, which then dries over the iron to create a protective barrier
32
explain how galvanising prevents rust formation
- zinc is more reactive than iron so will corrode in preference to the iron - this means that all the zinc must corrode before the iron begins rusting, preventing rust formation as it takes a long time for all the zinc to corrode away - this is both sacrificial protection and a barrier method as a physical barrier is created over the iron from the oxygen and water vapour in the air
33
name the advantages and disadvantages of galvanising
- A = both a form of barrier method and sacrificial protection, long-lasting - D = expensive as it costs a lot of money to heat zinc to its molten state due to its high melting point
34
what is sacrificial protection? explain how it prevents rust formation
- sacrificial protection = when a block of more reactive metal is placed onto the iron to prevent rust formation - this more reactive block of metal will corrode in preference to the iron and leave it intact for a long time as all the reactive metal must react before iron begins rusting
35
advantages and disadvantages of sacrificial protection
- A = effective, protects a very large surface - D = expensive, must be repeatedly replaced for continued protection once the more reactive metal has completely corroded
36
define oxidation
loss of electrons
37
define reduction
gain of electrons
38
OIL RIG
Oxidation Is Loss of electrons Reduction Is Gain of electrons
39
define redox reaction
a reaction in which reduction and oxidation take place simultaneously
40
define reducing agent
a substance that causes another substance to become reduced and in the process becomes oxidised
41
define oxidising agent
a substance that causes another substance to become oxidised, and in the process becomes reduced
42
how are most metals found underground?
most metals are found underground in ores which they need to be extracted out of (e.g. iron ores)
43
how are the most unreactive metals found underground?
unreactive metals such as copper, silver and gold are often found as the uncombined element underground
44
what determines the method through which a metal is extracted?
its position in the reactivity series
45
how are metals below hydrogen extracted?
- the metals below hydrogen (copper,silver,gold) are the 3 most unreactive metals in the reactivity series - this means that they can be physically mined out of the ground, as they exist naturally as uncombined pure metals underground
46
how is gold extracted?
- gold is below hydrogen + the least reactive metal in the reactivity series - this means that it exists as the uncombined, pure metal underground - this allows gold to be physically mined directly from the ground - this is a cheap + easy extraction method
47
how are metals below carbon extracted?
- metals below carbon in the reactivity series are extracted by being displaced out of their ore using carbon - ie Fe2O3 is reduced by carbon to become iron - expensive method of extraction as heat energy is required to heat the metal for the reduction reaction
48
how is iron extracted?
- iron is below carbon in the reactivity series - this means that carbon can displace the iron out of its iron ore in a reduction reaction by heating it
49
how are metals above carbon extracted?
- the metals above carbon are the most reactive metals in the reactivity series - this means that carbon cannot easily displace these metals out of their compounds/ores in a reduction reaction when heated - ∴, only electrolysis can be used to extract these metals in molten state, when ions are mobile in the compound - expensive as electricity is an expensive resource that is essential to electrolysis
50
how is aluminium extracted?
- aluminium is above carbon in the reactivity series - this means that carbon cannot easily displace the aluminium out of its ore/compound - ∴ only electrolysis can extract the Al metal from its ore (Al2O3 or bauxite) when molten, as ions are now mobile
51
uses of aluminium
- aeroplanes - electrical cables - cookware/packaging
52
uses of copper
- water pipes - electrical cables - cookware
53
uses of iron
too brittle to be used in its pure form
54
what is the alloy steel made of?
iron and carbon
55
uses of low-carbon steel
- nails - car bodies/ships - girders (construction)
56
uses of high-carbon steel
- cutting tools - masonry
57
uses of stainless steel
- cutlery - cookware - kitchen sinks
58
what properties make a metal or alloy suited for making aeroplanes?
- low density - unreactive
59
what properties make a metal or alloy suitable for making electrical cables?
- conducts electricity - ductile
60
what properties make a metal or alloy suitable for making cookware?
- unreactive - conducts heat
61
what properties make a metal or alloy suitable for making water pipes?
- malleable - unreactive
62
what properties make a metal or alloy suitable for making girders?
- strong - hard
63
define alloy
a mixture of a metal and one or more elements, usually other metals or carbon
64
why are alloys stronger and harder than pure metals?
- atoms in a pure metal are arranged in densely packed layers which can easily slide - this means that most pure metals are very soft - atoms of of other elements are of different sizes - these differently sized atoms distort the regular structure of the metal atoms, making it harder for layers to slide over one another - this makes alloys stronger and harder than pure metals

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