Unit 3a- Metal Reactivity

Question 1

Describe the main features of metals in terms of their structure

Answer 1

Positive metal ions arranged in layers with delocalised electrons

Question 2

Explain why metals can conduct electricity

Answer 2

Delocalised electrons are free to carry charge

Question 3

In terms of electrons, what do group 1 elements have in common?

Answer 3

1 electron in the outer shell

Question 4

Explain why the group 1 elements are called alkali metals

Answer 4

They are metals that form alkalis when they react with water

Question 5

What is a displacement reaction?

Answer 5

A reaction in which a more reactive element takes the place of a less reactive element in a compound

Question 6

Explain why potassium is more reactive than lithium (3 marks)

Answer 6

More shells/electrons, less shielding (or weaker attraction from nucleus), easier to lose electrons

Question 7

Explain why sodium is less reactive than caesium (3 marks)

Answer 7

Fewer shells/electrons, less shielding (or stronger attraction from nucleus), harder to lose electrons

Question 8

What is the reactivity series?

Answer 8

A list of elements ordered by their reactivity

Question 9

How can metals be placed in order of their reactivity?

Answer 9

Add the metals to water or acid and see which ones react the most (by how much fizzing there is)

Question 10

What is the name for a reaction where oxygen is removed from a compound?

Answer 10

Reduction

Question 11

What is the name for a reaction where oxygen is added to a compound?

Answer 11

Oxidation

Question 12

Explain why zinc can be extracted from zinc oxide with carbon but magnesium cannot be extracted from magnesium oxide with carbon

Answer 12

Magnesium is more reactive than carbon (1), Zinc is less reactive than carbon (1), Carbon can therefore remove oxygen from zinc oxide but not magnesium oxide (1)

Question 13

Explain why gold and silver can be found naturally in the Earth’s crust

Answer 13

It is very unreactive

Question 14

What process is used to extract metals more reactive than carbon

Answer 14

Electrolysis

Question 15

Define an ore

Answer 15

A material containing enough metal in it for it to be economically worthwhile to extract the metal.

Question 16

Define a displacement reaction

Answer 16

A reaction in which a more reactive element takes the place of a less reactive element in one of its compounds or in solution

Question 17

Define oxidation in the context of loss and gain of electrons

Answer 17

Oxidation is the loss of electrons

Question 18

Define reduction in the context of loss and gain of electrons

Answer 18

Reduction is the gain of electrons

Question 19

Which of the substances below has been oxidized and which has been reduced? Al³⁺ + Fe → Fe³⁺ + Al

Answer 19

Aluminium has been reduced and iron has been oxidised

Question 20

Show two half equations for the reaction below: Al³⁺ + Fe → Fe³⁺ + Al

Answer 20

Al³⁺ + 3e⁻ → Al, Fe → Fe³⁺ + 3e-

Question 21

What is the order of the reactivity series?

Answer 21

Group 1, Group 2, Group 3 Transition metals

Question 22

Which groups are more reactive than carbon?

Answer 22

Group 1, Group 2 and Group 3

Question 23

Which groups are less reactive than carbon?

Answer 23

Transition metals

Question 24

Which groups do we use electrolysis to extract the metal from the compound?

Answer 24

Group 1, 2 and 3

Question 25

Which group do we use carbon to reduce the metal oxdide?

Answer 25

Transition metals

Question 26

Metal + Oxygen ->?

Answer 26

Metal + Oxygen –> Metal oxide

Question 27

Metal + water -> ?

Answer 27

Metal + water -> metal hydroxide + hydrogen

Question 28

Metal + acid ->?

Answer 28

Metal + acid -> salt + water

Question 29

What is the test for hydrogen?

Answer 29

Give a squeaky pop with a lit splint