Paper 1 - Reactivity Series

Question 1

How can metals be arranged in a reactivity series based on their reactions
with water?

Answer 1

The more vigorous the reaction of metal with water, the higher up on the reactivity series it will be
- Reactive metals such as potassium, sodium, lithium and calcium all react very vigorously with water
- Less reactive metals only react with steam

Question 2

How can metals be arranged in a reactivity series based on their reactions
with dilute hydrochloric or sulfuric acid?

Answer 2

• The rate of reaction of a metal with a dilute acid can be used to work out its place in the reactivity series
• The faster the rate of reaction with acid, the more reactive the metal and the higher up on the reactivity series it is
• Very reactive metals react explosively

Question 3

How can metals be arranged in a reactivity series based on their displacement reactions between metals and metal oxides?

Answer 3

• More reactive metals react more strongly than less reactive metals
• So a more reactive metal will displace a less reactive metal; from its oxide because it will bond more strongly to the oxygen
• The metal that displaces other metals is the most reactive

Question 4

How can metals be arranged in a reactivity series based on their displacement reactions between metals and aqueous solutions of metal salts?

Answer 4

• More reactive metals react more strongly than less reactive metals
• If a more reactive metal is placed in a solution of a less reactive metal salt, the reactive metal will displace the less reactive metal in the salt.
• The metal that displaces other metals is the most reactive

Question 5

What is the reactivity series?

Answer 5

potassium
sodium
lithium
calcium,
magnesium
aluminium
zinc
iron
copper
silver
gold

Question 6

Under what conditions may iron rust?

Answer 6

When in contact with oxygen (from the air) and water

Question 7

How do barrier methods prevent the rusting of iron?

Answer 7

Plastic or Oil acts as a barrier between the iron and oxygen/water

Question 8

How does galvanising prevent the rusting of iron?

Answer 8

The coat of zinc on the iron will stop the iron from being oxidised as the Zinc will be oxidised instead as it is more reactive than iron

Question 9

How does sacrificial protection prevent the rusting of iron?

Answer 9

• A more reactive metal is placed with the iron
• The more reactive metal is oxidised instead of the iron

Question 10

What element is often used for sacrificial protection and galvanising?

Answer 10

Zinc

Question 11

What can barrier methods be used for?

Answer 11

• Painting/Coating with plastic can be used for big and small structures and can be decorative
• Oiling/Greasing must be used when moving parts are involved such as a bike chain

Question 12

Give 2 examples of when sacrificial protection can be used

Answer 12

Big blocks of zinc can be bolted into the iron on ships’ hulls or underground iron pipes

Question 13

What is oxidation in terms of gain or loss of oxygen?

Answer 13

Gain of oxygen

Question 14

What is reduction in terms of gain or loss of oxygen?

Answer 14

Loss of oxygen

Question 15

What does redox mean?

Answer 15

A redox reaction is a reaction a reaction involving the transfer of electrons

Question 16

What is a reducing agent in terms of gain or loss of oxygen?

Answer 16

• The substance that causes the metal to lose oxygen
• Reducing agent is oxidised and gains oxygen

Question 17

What is an oxidising agent in terms of gain or loss of oxygen?

Answer 17

• The substance that causes the metal to gain oxygen
• The oxidising agent is reduced and loses oxygen

Question 18

What is oxidation in terms of gain or loss of electrons?

Answer 18

Loss of electrons

Question 19

What is reduction in terms of in terms of gain or loss of electrons?

Answer 19

Gain of electrons

Question 20

What is a reducing agent in terms of gain or loss of electrons?

Answer 20

• The substance that causes the metal to gain electrons
• The reducing agent is oxidised and loses electrons

Question 21

What is an oxidising agent in terms of gain or loss of electrons?

Answer 21

• The substance that causes the metal to lose electrons
• Oxidising agent is reduced and gains electrons

Question 22

Describe a practical to investigate reactions between dilute hydrochloric and sulfuric acids and metals

Answer 22

• Set up 3 boiling tubes and fill them with equal volumes of dilute hydrochloric acid or sulfuric acid
• Then place pieces of magnesium, zinc and iron in separate test tubes and make sure the size and shape of the metal are the same
• The speed of reaction is indicated by the rate at which bubbles of hydrogen are given off
• The hydrogen is confirmed by the burning splint test
• The magnesium should give off the loudest squeaky pop as it has the most vigorous reaction producing the most hydrogen gas