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GCSE Chemistry COPY > C5.2 - Displacement reactions > Flashcards

C5.2 - Displacement reactions Flashcards

1
Q

You can use the reactions of metals with water and dilute acid to get an order of reactivity.
How can you also judge reactivity?

A

You can also judge reactivity by putting the metals ‘into competition’ with each other

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2
Q

You can judge reactivity by putting the metals ‘into competition’ with each other.
How can you do this?

A

You can judge reactivity by putting the metals ‘into competition’ with each other:

  1. One metal starts off as atoms of the element
  2. The other metal starts off as positive ions in a solution of one of its salts
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3
Q

Putting the metals ‘into competition’ with each other to judge reactivity:
One metal starts off as atoms of the element and the other metal starts off as positive ions in a solution of one of its salts.
Example

A

For example:
1.Magnesium metal, Mg (s)
2. Copper(II) ions, Cu2+ (aq)
,in a solution of copper(II) sulfate

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4
Q

What will a more reactive metal do?

A

A more reactive metal will displace a less reactive metal from an aqueous solution of one of its salts

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5
Q

Putting the metals ‘into competition’ with each other to judge reactivity:
One metal starts off as atoms of the element and the other metal starts off as positive ions in a solution of one of its salts.
For example, magnesium metal, Mg (s), and copper(II) ions, Cu2+ (aq), in a solution of copper(II) sulfate.
What will happen?

A

Magnesium is more reactive than copper, so the copper ions will be displaced from solution to form copper metal, Cu (s)

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6
Q

Putting the metals ‘into competition’ with each other to judge reactivity:
One metal starts off as atoms of the element and the other metal starts off as positive ions in a solution of one of its salts.
For example, magnesium metal, Mg (s), and copper(II) ions, Cu2+ (aq), in a solution of copper(II) sulfate.
Magnesium is more reactive than copper, so the copper ions will be displaced from solution to form copper metal, Cu (s).
What happens, in this reaction?

A

In this reaction, the magnesium metal:

  1. Forms aqueous magnesium ions, Mg2+ (aq)
  2. Dissolves into the solution
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7
Q

The word equation for magnesium metal, Mg (s), and copper(II) ions, Cu2+ (aq), in a solution of copper(II) sulfate

A

The word equation for magnesium metal, Mg (s), and copper(II) ions, Cu2+ (aq), in a solution of copper(II) sulfate is:
Magnesium + Copper(II) sulfate —> Magnesium sulfate + Copper

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8
Q

Magnesium + Copper(II) sulfate —> Magnesium sulfate + Copper.
The balanced symbol equation including state symbols

A

The balanced symbol equation including state symbols is:

Mg (s) + CuSO4 (aq) —> MgSO4 (aq) + Cu (s)

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9
Q

Displacement reaction

A

A displacement reaction is a reaction in which a more reactive element takes the place of a less reactive element in:

  1. One of its compounds
  2. Solution
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10
Q

Ionic equation

A 
An ionic equation is an equation that shows only those:
1. Ions
Or,
2. Atoms
that change in a chemical reaction
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11
Q

The ionic equation of Magnesium + Copper(II) sulfate —> Magnesium sulfate + Copper

A

The ionic equation of Magnesium + Copper(II) sulfate —> Magnesium sulfate + Copper is:
Mg (s) + Cu2+ (aq) —> Mg2+ (aq) + Cu (s)

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12
Q

Why is the ionic equation of Magnesium + Copper(II) sulfate —> Magnesium sulfate + Copper Mg (s) + Cu2+ (aq) —> Mg2+ (aq) + Cu (s)?

A

The ionic equation is of Magnesium + Copper(II) sulfate —> Magnesium sulfate + Copper is Mg (s) + Cu2+ (aq) —> Mg2+ (aq) + Cu (s), because the sulfate ions remain the same, so do not appear in the ionic equation

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13
Q

The chemical formula of sulfate ions

A

The chemical formula of sulfate ions is:

SO42-

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14
Q

The ionic equation is of Magnesium + Copper(II) sulfate —> Magnesium sulfate + Copper is Mg (s) + Cu2+ (aq) —> Mg2+ (aq) + Cu (s)
What does this show?

A

This shows that magnesium atoms have a greater tendency to form positive ions than copper atoms

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15
Q

Zinc in relation to lead

A

Zinc is:

  1. More reactive than lead
  2. Higher up the reactivity series than lead
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16
Q

Zinc is more reactive than lead and it is higher up the reactivity series.
Therefore, what does zinc do?

A

Therefore, zinc displaces lead from its solution

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17
Q

Chemical equation for:

Zinc + Lead nitrate —> Zinc nitrate + Lead

A

The chemical equation for Zinc + Lead nitrate —> Zinc nitrate + Lead is:
Zn (s) + Pb(NO3)2 (aq) —> Zn(NO3)2 (aq) + Pb (s)

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18
Q

Zinc is more reactive than lead - it is higher up the reactivity series.
Therefore, zinc displaces lead from its solution.
What would you see?

A

You would see the lead metal forming as crystals on the zinc

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19
Q

How can you include the non-metals hydrogen and carbon in the reactivity series?

A

You can include the non-metals:
1. Hydrogen
2. Carbon
in the reactivity series using displacement reactions

20
Q

You can include the non-metals hydrogen and carbon in the reactivity series using displacement reactions.
How can you think of the metal plus acid reactions?

A

You can think of the metal plus acid reactions as displacement of hydrogen ions from solution

21
Q

You can include the non-metals hydrogen and carbon in the reactivity series using displacement reactions.
You can think of the metal plus acid reactions as displacement of hydrogen ions from solution.
Copper cannot do what, whereas lead can?

A

Copper cannot displace the hydrogen from an acid, whereas lead can

22
Q

What can carbon be used in?

A

Carbon can be used in the extraction of metals from their oxides

23
Q

Carbon can be used in the extraction of metals from their oxides (another type of displacement reaction).
However, what can carbon only do this for?

A

Carbon can only do this for metals below aluminium in the reactivity series

24
Q

Carbon can be used in the extraction of metals from their oxides (another type of displacement reaction).
However, carbon can only do this for metals below aluminium in the reactivity series.
What does it not displace?

A

Carbon does not displace aluminium from aluminium oxide

25
Q

Carbon can be used in the extraction of metals from their oxides (another type of displacement reaction).
However, carbon can only do this for metals below aluminium in the reactivity series.
Carbon does not displace aluminium from aluminium oxide, but can displace zinc from zinc oxide.
So where is carbon placed in the reactivity series?

A

Carbon is placed between:
1. Aluminium
2. Zinc
in the reactivity series

26
Q

Oxidation

A

Oxidation is the:

  1. Chemical addition of oxygen
  2. Loss of electrons
27
Q

Reduction

A

Reduction is the:

  1. Removal of oxygen
  2. Gain of electrons
28
Q

Where is the reaction of the displacement of copper(II) ions by iron used?

A

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution

29
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The iron added to the copper sulfate solution is what iron?

A

The iron added to the copper sulfate solution is cheap scrap iron

30
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The ionic equation for this reaction

A

The ionic equation for the reaction of the displacement of copper(II) ions by iron is:
Fe (s) + Cu2+ (aq) —> Fe2+ (aq) + Cu (s)

31
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The ionic equation for the reaction of the displacement of copper(II) ions by iron is Fe (s) + Cu2+ (aq) —> Fe2+ (aq) + Cu (s).
What can you use to show what happens to each reactant?

A

You can use half-equations to show what happens to each reactant

32
Q

Half-equation

A

A half-equation is an equation that describes:
1. Reduction (gain of electrons)
Or,
2. Oxidation (loss of electrons)

33
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
What happens to the iron atoms?

A

The iron atoms lose 2 electrons to form iron(II) ions

34
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The iron atoms lose 2 electrons to form iron(II) ions (oxidation).
What do the 2 electrons from iron do?

A

The 2 electrons from iron are gained by the copper(II) ions as they form copper ions

35
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The iron atoms lose 2 electrons to form iron(II) ions (oxidation).
The 2 electrons from iron are gained by the copper(II) ions as they form copper ions.
What is this?

A

This is reduction (the gain of electrons)

36
Q

OILRIG

A

OILRIG:

  1. Oxidation Is Loss
  2. Reduction Is Gain
37
Q

You can use the reactions of metals with what to get an order of reactivity?

A

You can use the reactions of metals with:
1. Water
2. Dilute acid
to get an order of reactivity.

38
Q

Zinc is more reactive than lead and it is higher up the reactivity series.
Therefore, zinc displaces lead from its solution.
Zinc + Lead nitrate —> What?

A

Zinc + Lead nitrate —> Zinc nitrate + Lead

39
Q

You can include the non-metals hydrogen and carbon in the reactivity series using displacement reactions.
You can think of the metal plus acid reactions as displacement of hydrogen ions from solution.
Copper cannot displace the hydrogen from an acid, whereas lead can, so hydrogen is positioned where?

A

Copper cannot displace the hydrogen from an acid, whereas lead can, so hydrogen is positioned between:

  1. Copper
  2. Lead
40
Q

Carbon can be used in the extraction of metals from their oxides.
The extraction of metals from their oxides is another type of what?

A

The extraction of metals from their oxides is another type of displacement reaction

41
Q

Carbon can be used in the extraction of metals from their oxides (another type of displacement reaction).
However, carbon can only do this for metals below aluminium in the reactivity series.
Carbon does not displace aluminium from aluminium oxide, but can displace what?

A

Carbon does not displace aluminium from aluminium oxide, but can displace zinc from zinc oxide

42
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The ionic equation for the reaction of the displacement of copper(II) ions by iron is Fe (s) + Cu2+ (aq) —> Fe2+ (aq) + Cu (s).
You can use half-equations to show what happens to each reactant.
Fe (s) —> ?

A

Fe (s) —> Fe2+ (aq) + 2e-

43
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The iron atoms lose 2 electrons to form iron(II) ions.
This is what?

A

This is oxidation (the loss of electrons)

44
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The iron atoms lose 2 electrons to form iron(II) ions.
This is oxidation (the loss of electrons).
The iron atoms have been what?

A

The iron atoms have been oxidised

45
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The iron atoms lose 2 electrons to form iron(II) ions (oxidation).
The 2 electrons from iron are gained by the copper(II) ions as they form copper ions.
Cu2+ (aq) + 2e- —> ?

A

Cu2+ (aq) + 2e- —> Cu (s)

46
Q

The reaction of the displacement of copper(II) ions by iron is used in industry to extract copper metal from copper sulfate solution.
The iron atoms lose 2 electrons to form iron(II) ions (oxidation).
The 2 electrons from iron are gained by the copper(II) ions as they form copper ions.
This is reduction (the gain of electrons).
The copper(II) ions have been what?

A

The copper(II) ions have been reduced

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