Reactivity Series Flashcards
(104 cards)
1
Q
What is the reactivity series used for?
A
The reactivity series used to place a group of metals in order of reactivity based on the observations of their reactions with water and acids.
2
Q
Metal X reacts vigorously with acid, metal Y reacts violently with acid. Which is more hazardous/dangerous?
A
Metal Y because it reacts violently with acid.
3
Q
Which Metal reacts violently with water?
A
Potassium
4
Q
Which metal reacts less strongly with water?
A
Calcium
5
Q
Which metals react with very slowly with COLD water to the point where it isn’t considered a reaction?
A
Magnesium, Zinc and Iron
6
Q
Which metals don’t react with water at all?
A
Only Metals below Tin don’t react with water at all.
7
Q
Which metals react violently with acids?
A
Potassium, Sodium and Lithium
8
Q
Which metals react vigorously with acids?
A
Calcium and Magnesium
9
Q
Which metals react less strongly with acids?
A
Zinc, Iron, Tin and Lead
10
Q
How would metals placed high on the reactivity series react with acids?
A
Metals that are placed high on the reactivity series are very dangerous and so would react explosively with acids. The reaction would be very dangerous and the reaction would most likely not be done.
11
Q
What is formed when a metal reacts with an acid?
A
A salt and hydrogen gas
12
Q
Which metals do not react with acids at all?
A
Metals below Hydrogen do not react with acids at all.
13
Q
Which metals do not react with water or acids? Give examples
A
Copper, Silver, Gold and Platinum
14
Q
Which metal can be found in Earth?
A
Gold
15
Q
Which metals react with Steam?
A
Magnesium, Aluminum, Zinc and Iron
16
Q
Which Metal does not react with Oxygen?
A
Gold
17
Q
Give two ways we can compare reactivities of metals in an experiment.
A
You can watch how quickly bubbles of hydrogen gas are formed, considering that the more reactive the metal = the more rapidly bubbles will form. You can also measure the temperature change of the reaction in a set time period as the more reactive the metal, the greater the temperature change should be.
18
Q
When comparing the reactivities of metals in an experiment, what should be the control variables? (Things kept the same)
A
The mass and surface area are the control variables as they must be kept the same each time in order for the experiment to be fair.
19
Q
Describe how unreactive metals react.
A
They react more slowly in chemical reactions or don’t react at all.
20
Q
Give another purpose for displacement reactions
A
Displacement reactions can also be used to extract metals from their oxides/cores.
21
Q
Where is Carbon in the reactivity series?
A
Carbon is between Aluminum and Zinc in the reactivity series.
22
Q
What metals can Carbon extract from their oxides/core?
A
Carbon can only extract metals below it in the reactivity series.
23
Q
Which metals can Carbon not extract from their oxides/cores?
A
Carbon cannot extract metals above it from their oxides/cores as they are above Carbon in the reactivity series.
24
Q
How are metals that cannot be extracted from their oxides/cores by Carbon extracted?
A
By electrolysis
25
What should you say when asked why a metal should NOT be used in an experiment?
State that the metal is very reactive and the experiment would be dangerous.
26
Give a reason why one of the results in an experiment investigating the reactivity of metals might be lower than expected (an anomalous result)
This could be because a lower mass of metal was added.
27
Metals react with acids to produce what (what can be observed?)
Bubbles of gas would be produced/seen.
28
How can we prove that a chemical reaction has taken place?
State that a new substance has been formed and note any observational changes (colour change, change in state of matter, etc. etc.)
29
What is produced when a metal reacts with an acid?
A salt and a hydrogen gas
30
Metals below Carbon don’t react with cold water but instead react with…
Instead they react with steam
31
When a metal below Calcium reacts with steam, what is formed?
A metal oxide and hydrogen gas
32
What is an alloy?
An alloy is a metal containing two or more metallic elements to give a greater strength/resistance to corrosion.
33
Give a use for Copper
Electrical wiring
34
Why are metals sometimes used as alloys?
They are harder and keep their shape better.
35
If a metal cannot be extracted from its core/oxide by Carbon, the where is its position in the reactivity series?
Its position is above Carbon in the reactivity series
36
If a metal reacts with an acid, then where is its position in the reactivity series?
It is above Hydrogen in the reactivity series.
37
Why are there attractive forces in a metallic structure?
There are attractive forces in a metallic structure due to the the attractive forces between the positive ions and negative ions. Only opposite charges attract.
38
Give the order of the reactivity series (include Carbon and Hydrogen)
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminum
(Carbon)
Zinc
Iron
Tin
Lead
(Hydrogen)
Copper
Silver
Gold
Platinum
39
What is meant by a metal displacement reaction?
A more reactive metal will displace a less reactive metal from its compounds.
40
Give observations for a displacement reaction between metals & aqueous solutions of metal salts
The more reactive metal slowly disappears from the solution and displaces the less reactive metal.
41
Give two examples of displacement reactions.
- Reacting a metal with a metal oxide (by heating).
- Reacting a metal with an aqueous solution of a metal compound.
42
What is rusting?
Rusting is a chemical reaction between iron, water and oxygen to form hydrated iron(III)oxide.
43
What must be present for rust to occur?
Oxygen and water must be present for rusting to occur.
44
What type of process is rusting?
Rusting is a redox process.
45
What factors aggravate (speed up) rusting?
Salt and acid
46
Why does salty water aggravate rusting?
Salt water aggravates rusting due to the presence of sodium chloride in the salty water.
47
What exactly is rust?
It is a soft red-brown solid that flakes off the surface of iron easily.
48
Write the word equation for rust
Iron + Water + Oxygen → Hydrated Iron(III) Oxide
49
Write the balanced chemical equation for rust (reactants and products, include state symbols!)
4Fe (s) + 3O2 (g) + xH2O (l) → 2Fe2O3.xH2O (s)
50
What is another name for rust?
Hydrated Iron (III) Oxide
51
What is the formula (not equation) rust?
Fe2O3.xH2O
52
What is the formula (not equation) for Iron oxide?
Fe2O3
53
If a nail is left in air and water, what will occur?
It would rust as it is in contact with both air (which contains oxygen) and water. Therefore, both factors are present and rusting can take place.
54
If a nail is left in boiled water topped with a layer of oil, what will occur?
It will not rust as the nail is not in contact with Oxygen. The boiled water doesn’t contain oxygen and the oil keeps Oxygen out by acting as a barrier.
55
If a nail is left in air and Calcium Chloride, what will occur?
The nail would not rust as it is not in contact with water, water/moisture is needed for rusting (as calcium chloride is a drying agent it absorbs any water molecules present).
56
What do the results of the iron nail experiment show?
The results show that both Oxygen and water must be present for rusting to occur.
57
What happens when rust flakes off the surface of iron?
It exposes fresh iron below which then undergoes rusting.
58
What are the two ways we can prevent rust?
Barrier methods and Sacrificial Protection/Galvanizing
59
Explain barrier methods in general
Barrier methods prevent rust by coating iron with barriers that prevent the iron from coming into contact with water and oxygen.
60
What are some common barrier methods?
Painting, greasing (using oil) and plastic coating
61
What are the disadvantages of barrier methods?
If the coatings are washed away or scratched, the iron is once again exposed to water and oxygen and will rust
62
Explain galvanising
Galvanising is a process where the iron to be protected is coated with a layer of zinc. Zinc Carbonate (ZnCO3) is formed when zinc reacts with oxygen and carbon dioxide in the air and protects the iron by the barrier method. If the coating is damaged or scratched, the iron is still protected from rusting because zinc preferentially corrodes as it is higher up the reactivity series than iron
63
What are the advantages of galvanising?
If the coating is damaged or scratched, the iron is still protected from rusting because zinc preferentially corrodes as it is higher up the reactivity series than iron.
64
What does rust do to iron structures?
It flakes off the surface of iron easily, exposing fresh iron below which then undergoes rusting, meaning that over time all of the iron rusts and its structure becomes weakened.
65
Explain sacrificial corrosion/protection
Sacrificial corrosion occurs when a more reactive metal is intentionally allowed to corrode.
66
Give an example of sacrificial corrosion/protection
An example of this occurs with ships’ hulls which sometimes have large blocks of magnesium or magnesium alloys attached.
67
Explain what happens to the ships’ hulls that have large blocks of magnesium/magnesium alloys attached
The blocks slowly corrode and provide protection to the hull by pushing electrons onto the iron which prevents it from being reduced to iron(III) ions.
68
What is corrosion?
Corrosion is the general term used to describe the degradation of metal surfaces.
69
What is rusting?
Rusting is the specific type of corrosion that happens to iron.
70
Explain, in your own words, why zinc protects iron/reacts instead of it when the coating is scratched.
When the layer of zinc is scratched, the iron is still protected from rusting because Zinc preferentially corrodes as it is higher up the reactivity series than iron . This is because Zinc pushes electrons onto the iron and the iron accepts the electrons released by zinc and this stops the iron reacting with the oxygen.
71
What can the reaction of metals with oxygen be classified as?
It can be classified as oxidation.
72
What is Oxidation (in terms of Oxygen)?
Oxidation is any reaction in which a substance gains oxygen.
73
What is the opposite of Oxidation?
The opposite of oxidation is reduction.
74
What is reduction in terms of Oxygen?
Reduction is a reaction in which a substance loses oxygen.
75
Displacement reactions can be classified as…
A redox reaction
76
What is a redox reaction?
A redox reaction is when oxidation and reduction occur in the same reaction, simultaneously.
77
Why is it called a redox reaction?
Oxidation cannot occur without reduction happening simultaneously, hence these are called redox reactions.
78
What is an Oxidising agent?
A species which brings about oxidation by gaining electrons/losing Oxygen. The oxidising agent is itself reduced.
79
What is a reducing agent?
A species which brings about reduction by losing electrons/gaining Oxygen. The reducing agent is itself oxidised.
80
What do spectator ions do?
They appear on both sides of the equation unchanged and do not participate in the chemistry of the reaction so can be omitted (left out).
81
What is the mnemonic to help remember the definitions of oxidation and reduction (in terms of electrons)?
O: Oxidation
I: is
L: Loss of Electrons
R: Reduction
I: is
G: Gain of Electrons
82
Why is it difficult to place Aluminum in the reactivity series?
It is difficult to place Aluminum in the reactivity series due to formation of aluminium oxide layer on the metal surface making it appear less reactive than it is. Once this layer is removed more reliable observations can be made.
83
Describe the reaction of the metals with water
Potassium reacts violently, Sodium reacts quickly; Calcium reacts less strongly
84
Which metal reacts quickly with water?
Sodium
85
Describe the reactions of the metals with acid.
Potassium reacts violently; Sodium reacts violently, Calcium and Magnesium reacts vigorously; Zinc and Iron reacts less strongly.
86
Only metals above - in the reactivity series will react with - -.
Only metals above Hydrogen in the reactivity series will react with dilute acids.
87
The more - the metals, then the more - the - will be.
The more reactive the metals, then the more vigorous the reaction will be.
88
Write the chemical equation for the reaction of Magnesium with Sulphuric Acid
Mg + H2SO4 -> MgSO4 + H2
89
Write the chemical equation for the reaction of Zinc with Sulphuric Acid
Zn + H2SO4 -> ZnSO4 + H2
90
Write the chemical equation for the reaction of Iron with Sulphuric Acid
Fe + H2SO4 -> FeSO4 + H2
91
Write the chemical equation for Magnesium and Hydrochloric Acid
Mg + 2HCL -> MgCl2 + H2
92
Write the chemical equations for Zinc and Hydrochloric Acid
Zn + 2HCI -> ZnCl2 + H2
93
Write the chemical equations for Iron and Hydrochloric Acid
Fe + 2HCl -> FeCl2 + H2
94
The reactivity of metals decreases going down the reactivity series, what does this mean?
This means that a more reactive metal will displace a less reactive metal from its compound.
95
How can you reduce copper (II) oxide? What is the reducing agent and what is the the oxidising agent? Write a word and chemical equation for the reaction.
It is possible to reduce copper(II) oxide by heating it with zinc.
The reducing agent in the reaction is zinc and the oxidising agent is Copper (II).
Zn + CuO → ZnO + Cu
zinc + copper(II) oxide → zinc oxide + copper
96
The reactivity between two between metals can be compared using
- - in- - of one of the metals.
The reactivity between two between metals can be compared using
Displacement reactions in salt solutions of one of the metals.
97
What is the results of Magnesium displacing copper (II) sulfate solution?
The blue colour of the CuSO4 solution fades as colourless magnesium sulfate solution is formed
Copper coats the surface of the magnesium and also forms solid metal which falls to the bottom of the beaker.
98
Method to investigate rusting
Set up three test tubes each with an iron nail inside.
The first test tube contains air and water.
The water in the second test tube is boiled to remove any dissolved oxygen.
The oil provides a barrier to prevent oxygen diffusing into the boiled water
Calcium chloride is a drying agent in the third test tube.
Leave the apparatus for a few days to give it time to react.
99
What is formed when Zinc reacts with oxygen and carbon dioxide in the air? If the coating of zinc was damaged/scratched is the iron still protected from rusting and why?
ZnCO3 is formed when zinc reacts with oxygen and carbon dioxide in the air and protects the iron by the barrier method
If the coating is damaged or scratched, the iron is still protected from rusting because zinc preferentially corrodes as it is higher up the reactivity series than iron.
100
Displacement reactions can be
analysed in terms of - - by studying the transfer of
by -.
Displacement reactions can be
analysed in terms of redox reactions by studying the transfer of
by electrons.
101
What does the reactivity of metals depend on?
It depends on how easily they lose electrons and form positive ions.
102
What is the the only other metal (besides iron) can we say “rusts”? And why?
The only other metal (besides iron) we can say “rusts” is steel, this is because it is an alloy made from iron.
103
Explain why aluminium window frames do not corrode after they are made.
Aluminum has a coating of aluminum oxide, so the aluminium oxide protects the metal from further corrosion.
104
Why is useful to place Carbon and Hydrogen into the reactivity series?
It is useful to place Carbon and Hydrogen into the reactivity series, because these elements can be used to extract metals.
