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GCSE Chemistry > Reactivity Series > Flashcards

Reactivity Series Flashcards

1
Q

What does the reactivity of metals determine?

A

Their reaction with water or dilute acids.

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2
Q

What gas is produced when reactive metals react with dilute acids?

A

Hydrogen.

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3
Q

How can hydrogen gas be tested?

A

By holding a lit splint near the gas; a ‘squeaky pop’ sound confirms its presence.

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4
Q

What is the reactivity series order of metals from most reactive to least reactive?

A

Potassium, sodium, lithium, calcium, magnesium, aluminum, carbon, zinc, iron, hydrogen, copper, silver, gold.

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5
Q

What happens when a reactive metal reacts with a dilute acid?

A

A salt and hydrogen gas are produced.

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6
Q

How is the name of a salt formed?

A

The metal provides the first part

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7
Q

What salt is formed from hydrochloric acid?

A

A chloride.

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8
Q

What salt is formed from sulfuric acid?

A

A sulfate.

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9
Q

What salt is formed from nitric acid?

A

A nitrate.

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10
Q

What was the purpose of the investigation?

A

To investigate the reactivity of magnesium

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11
Q

What was the independent variable in the investigation to determine reactivity?

A

The type of metal used (magnesium

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12
Q

What was the dependent variable in the investigation to determine reactivity?

A

The volume of hydrogen gas produced when each metal reacted with dilute hydrochloric acid.

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13
Q

How was the dependent variable measured in the investigation to determine reactivity?

A

By collecting the hydrogen gas produced using a gas syringe or a measuring cylinder (units: cm³).

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14
Q

What was the purpose of the investigation?

A

To investigate the reactivity of magnesium, aluminum, zinc, iron, and copper by reacting them with dilute hydrochloric acid and measuring hydrogen gas production.

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15
Q

What was the independent variable in the investigation to determine reactivity?

A

The type of metal used (magnesium, zinc, iron, or copper).

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16
Q

What was the dependent variable in the investigation to determine reactivity?

A

The volume of hydrogen gas produced when each metal reacted with dilute hydrochloric acid.

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17
Q

How was the dependent variable measured in the investigation to determine reactivity?

A

By collecting the hydrogen gas produced using a gas syringe or a measuring cylinder (units: cm³).

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18
Q

What were the control variables in the investigation to determine reactivity of metals?

A

Concentration of hydrochloric acid, volume of hydrochloric acid, and mass of the metal used.

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19
Q

Why was the concentration of hydrochloric acid kept constant in the investigation to determine reactivity of metals?

A

To ensure that differences in hydrogen gas production were due to the reactivity of the metals and not variations in acid concentration.

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20
Q

How was the concentration of hydrochloric acid kept constant in the investigation to determine reactivity of metals?

A

By using hydrochloric acid with the same molarity for all trials.

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21
Q

Why was the volume of hydrochloric acid kept constant in the investigation to determine reactivity of metals?

A

To ensure that all metals reacted with the same amount of acid

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22
Q

How was the volume of hydrochloric acid kept constant in the investigation to determine reactivity of metals?

A

By measuring and using the same volume of acid (e.g., 50 cm³) for each reaction.

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23
Q

Why was the mass of the metal kept constant in the investigation to determine reactivity of metals?

A

To ensure that the amount of hydrogen gas produced was determined only by the reactivity of the metal and not the quantity of metal used.

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24
Q

How was the mass of the metal kept constant in the investigation to determine reactivity of metals?

A

By using equal masses of each metal (e.g., 1 g).

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25
Q

What gas is formed when reactive metals are added to acids?

A

Hydrogen.

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26
Q

What is the independent variable in the investigation of metal reactivity with acids?

A

The type of metal used

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27
Q

What is the dependent variable in the investigation of metal reactivity with acids?

A

The volume of hydrogen gas produced or the temperature change measured in °C.

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28
Q

What are the controlled variables in the investigation of metal reactivity with acids?

A

Concentration of the acid, volume of acid, and mass of the metal.

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29
Q

How are controlled variables kept constant in the investigation of metal reactivity with acids?

A

By using the same concentration and volume of acid and the same mass of the metal samples.

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30
Q

What hazards are associated with the investigation of metal reactivity with acids?

A

Broken glass from the apparatus and dilute acid causing irritation to skin or eyes.

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31
Q

What precautions should you take during the investigation of metal reactivity with acids?

A

Wear safety goggles, handle glassware carefully, and wash skin if it comes into contact with acid.

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32
Q

What is the method for investigating the reactivity of metals with acids?

A

Measure 10 cm³ of acid into a boiling tube, record the initial temperature of the acid, add small pieces of the metal sample to the acid, and record the temperature change and any observations.

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33
Q

Which metals reacted in the investigation of metal reactivity with acids?

A

Magnesium aluminum, zinc, and iron.

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34
Q

Why did copper not react in the investigation of metal reactivity with acids?

A

Copper is too unreactive.

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35
Q

Why does aluminum sometimes show no reaction in the investigation of metal reactivity with acids?

A

It forms a protective oxide layer that prevents the acid from reacting with the aluminum.

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36
Q

Was the practical effective at judging metal reactivity in the investigation of metal reactivity with acids?

A

Partially effective; aluminum’s protective oxide layer caused inconsistent results.

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37
Q

How could you improve the investigation of metal reactivity with acids?

A

Clean the metals beforehand to remove oxide layers, repeat the experiment to improve reliability, and increase the concentration of the acid.

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38
Q

Which metal was the most reactive in the investigation of metal reactivity with acids?

A

Calcium.

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39
Q

Which metal was the least reactive in the investigation of metal reactivity with acids?

A

Copper.

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40
Q

How can you tell calcium is the most reactive in the investigation of metal reactivity with acids?

A

It produced the most bubbles in the test tube diagram and reacted the fastest.

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41
Q

Complete the word equation for the reaction of magnesium with sulfuric acid.

A

Magnesium + sulfuric acid → magnesium sulfate + hydrogen.

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42
Q

Complete the word equation for the reaction of calcium with hydrochloric acid.

A

Calcium + hydrochloric acid → calcium chloride + hydrogen.

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43
Q

Complete the word equation for the reaction of zinc with sulfuric acid.

A

Zinc + sulfuric acid → zinc sulfate + hydrogen.

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44
Q

Complete the word equation for the reaction of iron with nitric acid.

A

Iron + nitric acid → iron(II) nitrate + hydrogen.

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45
Q

Why is no reaction observed when aluminum is added to acid?

A

The oxide layer on aluminum prevents the acid from reacting with the metal.

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46
Q

What happens when solid zinc is added to copper(II) sulfate solution?

A

Zinc displaces copper

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47
Q

Word equation for the reaction between zinc and copper(II) sulfate solution

A

Zinc + Copper(II) sulfate → Zinc sulfate + Copper.

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48
Q

Chemical equation for the reaction between zinc and copper(II) sulfate solution

A

Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s).

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49
Q

Observation when magnesium is added to copper(II) sulfate solution

A

Copper is displaced forming a red-brown solid

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50
Q

Observation when magnesium is added to iron(II) sulfate solution

A

Iron is displaced forming a grey solid

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51
Q

Observation when magnesium is added to zinc sulfate solution

A

No reaction occurs.

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52
Q

Why do metals not react with solutions of their own salts?

A

The metal is already present in the salt solution and cannot displace itself.

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53
Q

Observation when zinc is added to magnesium sulfate solution

A

No reaction occurs.

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54
Q

Observation when zinc reacts with copper(II) sulfate solution

A

Copper is displaced forming a red-brown solid

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55
Q

Observation when zinc reacts with iron(II) sulfate solution

A

Iron is displaced forming a grey solid

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56
Q

Observation when copper is added to magnesium sulfate solution

A

No reaction occurs.

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57
Q

Observation when copper is added to zinc sulfate solution

A

No reaction occurs.

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58
Q

Observation when copper is added to iron(II) sulfate solution

A

No reaction occurs.

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59
Q

Observation when iron is added to magnesium sulfate solution

A

No reaction occurs.

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60
Q

Observation when iron reacts with copper(II) sulfate solution

A

Copper is displaced forming a red-brown solid

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61
Q

Observation when iron reacts with zinc sulfate solution

A

No reaction occurs.

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62
Q

Why is there no reaction between magnesium and magnesium sulfate?

A

Metals cannot displace themselves.

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63
Q

Order of metal reactivity based on observations

A

Magnesium > Zinc > Iron > Copper.

64
Q

Word equation for magnesium reacting with zinc sulfate

A

Magnesium + Zinc sulfate → Magnesium sulfate + Zinc.

65
Q

Chemical equation for magnesium reacting with zinc sulfate

A

Mg(s) + ZnSO₄(aq) → MgSO₄(aq) + Zn(s).

66
Q

Word equation for magnesium reacting with copper(II) sulfate

A

Magnesium + Copper(II) sulfate → Magnesium sulfate + Copper.

67
Q

Chemical equation for magnesium reacting with copper(II) sulfate

A

Mg(s) + CuSO₄(aq) → MgSO₄(aq) + Cu(s).

68
Q

Word equation for zinc reacting with iron(II) sulfate

A

Zinc + Iron(II) sulfate → Zinc sulfate + Iron.

69
Q

Chemical equation for zinc reacting with iron(II) sulfate

A

Zn(s) + FeSO₄(aq) → ZnSO₄(aq) + Fe(s).

70
Q

Word equation for zinc reacting with copper(II) sulfate

A

Zinc + Copper(II) sulfate → Zinc sulfate + Copper.

71
Q

Chemical equation for zinc reacting with copper(II) sulfate

A

Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s).

72
Q

Word equation for copper reacting with magnesium sulfate

A

Copper + Magnesium sulfate → No reaction.

73
Q

Word equation for copper reacting with iron(II) sulfate

A

Copper + Iron(II) sulfate → No reaction.

74
Q

Word equation for iron reacting with copper(II) sulfate

A

Iron + Copper(II) sulfate → Iron(II) sulfate + Copper.

75
Q

Chemical equation for iron reacting with copper(II) sulfate

A

Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s).

76
Q

Metal displacement reactions occur between which substances?

A

Metals and aqueous solutions of metal salts

77
Q

What happens when a more reactive metal is added to a solution of a less reactive metal salt?

A

The more reactive metal displaces the less reactive metal from its compound

78
Q

What are the observations when zinc is added to copper(II) sulfate solution?

A

Zinc remains grey

79
Q

Why don’t metals react with their own salts?

A

Because a metal cannot displace itself from a compound

80
Q

What is a displacement reaction?

A

A reaction where a more reactive element replaces a less reactive element in a compound

81
Q

What is oxidation in terms of oxygen?

A

Gain of oxygen

82
Q

What is reduction in terms of oxygen?

A

Loss of oxygen

83
Q

What is a redox reaction?

A

A reaction in which both oxidation and reduction occur

84
Q

What is an oxidizing agent?

A

A substance that causes oxidation by gaining electrons

85
Q

What is a reducing agent?

A

A substance that causes reduction by losing electrons

86
Q

What are the observations in the reaction between aluminum and iron(III) oxide?

A

Very bright light

87
Q

Is the thermite reaction exothermic or endothermic?

A

Exothermic as lots of heat is given out

88
Q

What is the word equation for the thermite reaction?

A

Aluminum + iron oxide → iron + aluminum oxide

89
Q

What is the balanced symbol equation for the thermite reaction?

A

2Al + Fe₂O₃ → 2Fe + Al₂O₃

90
Q

Why does the thermite reaction occur?

A

Aluminum is more reactive than iron so it displaces iron from its oxide

91
Q

What would happen if iron metal was heated with aluminum oxide?

A

No reaction as aluminum is already in a compound and is more reactive than iron

92
Q

What is electrolysis?

A

Electrolysis is the process of using electricity to break down a compound into its elements.

93
Q

How are metals arranged in the reactivity series?

A

Metals are arranged based on their ability to displace other metals in reactions.

94
Q

What is a displacement reaction?

A

A reaction where a more reactive metal replaces a less reactive metal in a compound.

95
Q

What is oxidation?

A

Oxidation is the loss of oxygen or gain of electrons.

96
Q

What is reduction?

A

Reduction is the gain of oxygen or loss of electrons.

97
Q

What is a redox reaction?

A

A reaction in which both oxidation and reduction occur.

98
Q

What is an oxidising agent?

A

A substance that causes another substance to be oxidised while it is reduced.

99
Q

What is a reducing agent?

A

A substance that causes another substance to be reduced while it is oxidised.

100
Q

What happens in the reaction between aluminium and iron(III) oxide?

A

Aluminium displaces iron from iron(III) oxide

101
Q

What is the word equation for the reaction between aluminium and iron(III) oxide?

A

Aluminium + Iron(III) Oxide → Iron + Aluminium Oxide

102
Q

What is the balanced symbol equation for the reaction between aluminium and iron(III) oxide?

A

2Al + Fe₂O₃ → 2Fe + Al₂O₃

103
Q

Is the thermite reaction exothermic or endothermic?

A

Exothermic

104
Q

What is the thermite reaction used for?

A

It is used to weld railway and tram tracks together.

105
Q

What would happen if iron metal was heated with aluminium oxide?

A

No reaction would occur because iron is less reactive than aluminium.

106
Q

What happens in the reaction between magnesium oxide and sodium?

A

Sodium displaces magnesium from magnesium oxide

107
Q

What is the balanced symbol equation for the reaction between magnesium oxide and sodium?

A

MgO + 2Na → Na₂O + Mg

108
Q

What happens in the reaction between copper(II) oxide and magnesium?

A

Magnesium displaces copper from copper(II) oxide

109
Q

What is the balanced symbol equation for the reaction between copper(II) oxide and magnesium?

A

CuO + Mg → MgO + Cu

110
Q

What happens in the reaction ZnO + C → Zn + CO?

A

Zinc oxide is reduced to zinc

111
Q

What happens in the reaction MgO + Na → Mg + Na₂O?

A

Magnesium oxide is reduced to magnesium

112
Q

What happens in the reaction CuO + H₂ → Cu + H₂O?

A

Copper(II) oxide is reduced to copper

113
Q

What happens in the reaction Fe₂O₃ + 3CO → 2Fe + 3CO₂?

A

Iron(III) oxide is reduced to iron

114
Q

What happens in the reaction PbO + 2CO → Pb + 2CO₂?

A

Lead(II) oxide is reduced to lead

115
Q

What is an ore?

A

A rock that contains a metal compound.

116
Q

How can carbon be used to extract metals?

A

Carbon can be used to reduce metal oxides if the metal is less reactive than carbon.

117
Q

Why is electrolysis used for some metals instead of reduction with carbon?

A

Metals more reactive than carbon cannot be extracted by reduction and must be extracted using electrolysis.

118
Q

What happens in a redox reaction?

A

Oxidation and reduction occur simultaneously.

119
Q

What is the definition of reduction in terms of electrons and oxygen?

A

Reduction is the gain of electrons or the loss of oxygen.

120
Q

What is the definition of oxidation in terms of electrons and oxygen?

A

Oxidation is the loss of electrons or the gain of oxygen.

121
Q

What is the function of a reducing agent in a reaction?

A

A reducing agent causes another substance to be reduced and is itself oxidized.

122
Q

What is the function of an oxidizing agent in a reaction?

A

An oxidizing agent causes another substance to be oxidized and is itself reduced.

123
Q

Will magnesium react with magnesium oxide?

A

No

124
Q

Will sodium react with magnesium oxide?

A

Yes

125
Q

What is the balanced equation for the reaction between magnesium oxide and sodium?

A

MgO + 2Na → Na₂O + Mg.

126
Q

Which element is oxidized when magnesium oxide reacts with sodium?

A

Sodium.

127
Q

Which element is reduced when magnesium oxide reacts with sodium?

A

Magnesium.

128
Q

Will iron react with zinc oxide?

A

No

129
Q

Will magnesium react with copper(II) oxide?

A

Yes

130
Q

What is the balanced equation for the reaction between copper(II) oxide and magnesium?

A

CuO + Mg → MgO + Cu.

131
Q

Which element is oxidized when copper(II) oxide reacts with magnesium?

A

Magnesium.

132
Q

Which element is reduced when copper(II) oxide reacts with magnesium?

A

Copper.

133
Q

What is the oxidizing agent in the reaction ZnO + C → Zn + CO?

A

ZnO.

134
Q

What is the reducing agent in the reaction ZnO + C → Zn + CO?

A

C.

135
Q

What is the oxidizing agent in the reaction MgO + Na → Mg + Na₂O?

A

MgO.

136
Q

What is the reducing agent in the reaction MgO + Na → Mg + Na₂O?

A

Na.

137
Q

What is the oxidizing agent in the reaction CuO + H₂ → Cu + H₂O?

A

CuO.

138
Q

What is the reducing agent in the reaction CuO + H₂ → Cu + H₂O?

A

H₂.

139
Q

What is the oxidizing agent in the reaction CuO + C → Cu + CO?

A

CuO.

140
Q

What is the reducing agent in the reaction CuO + C → Cu + CO?

A

C.

141
Q

What is the oxidizing agent in the reaction ZnO + CO → Zn + CO₂?

A

ZnO.

142
Q

What is the reducing agent in the reaction ZnO + CO → Zn + CO₂?

A

CO.

143
Q

What is the oxidizing agent in the reaction Fe₂O₃ + 3CO → 2Fe + 3CO₂?

A

Fe₂O₃.

144
Q

What is the reducing agent in the reaction Fe₂O₃ + 3CO → 2Fe + 3CO₂?

A

CO.

145
Q

What is the oxidizing agent in the reaction PbO + 2CO → Pb + 2CO₂?

A

PbO.

146
Q

What is the reducing agent in the reaction PbO + 2CO → Pb + 2CO₂?

A

CO.

147
Q

What is an ore?

A

A rock that contains a metal compound in sufficient amounts to make extraction worthwhile.

148
Q

How does carbon extract metals from metal oxides?

A

Carbon reduces the metal oxide by removing oxygen

149
Q

When can carbon be used to extract a metal from its ore?

A

When the metal is less reactive than carbon.

150
Q

What extraction method is used if the metal is more reactive than carbon?

A

Electrolysis.

151
Q

What is electrolysis?

A

A process that uses electricity to decompose a compound into its elements.

152
Q

What are the steps for extracting copper using carbon?

A

Mix copper(II) oxide with carbon

153
Q

What is the observation of copper(II) oxide before heating?

A

Black solid.

154
Q

What is the observation of carbon before heating?

A

Black solid.

155
Q

What is the observation of the reaction mixture after heating?

A

Black powder and orange/pink solid (copper).

GCSE Chemistry (8 decks)

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