Displacement Reactions

Question 1

When does a displacement reaction occur?

Answer 1

When a solid metal is placed in a solution of ions of a different metal. The solid metal can displace the metal in the solution if it (the solid metal) is more reactive

Question 2

What happens if the solid metal is less reactive?

Answer 2

There will be no reaction

Question 2

Explain how a displacement reaction works using the example of Fe(s) + CuSO₄(aq)

Answer 2

In a successful displacement reaction, the solid metal will become a cation (solution) and the solution will become a solid metal.
Fe(s) + CuSO₄(aq) –> Cu(s) + FeSO₄(aq)
Fe is more reactive than Cu and displaces it from the solution. Solid Cu forms on the surface of the solid Fe and some of the Fe dissolves into the solution

Question 2

Mg + FeSO –>

Answer 2

Fe + MgSO

Question 3

AgO + Cu –>

Answer 3

CuO + Ag

Question 4

What is extraction?

Answer 4

The process of removing the metal from its ore (compound it is found in) by giving electrons to a metal ion to return it to its solid form

Question 5

The more reactive a metal, the (harder/easier) it is to extract it from its ore

Answer 5

Harder

Question 6

How does extraction with carbon work?

Answer 6

Metals which are below carbon on the activity series can be extracted with carbon. The carbon removes the carbon from the metal ore, forming carbon dioxide and the pure form of the metal
Eg. Iron oxide + carbon monoxide –> iron + carbon dioxide

Question 6

What are native metals?

Answer 6

They are the least reactive metals and therefore can exist in their solid and pure form in nature. They are at the bottom of the activity series. Examples: silver, gold, platinum

Question 7

How does extraction with electrolysis work?

Answer 7

Metals which are above carbon on the activity series can be extracted via electrolysis.
An electrical current is passed through a molten form of the ore, resulting in the extraction of the pure form of the metal.
This process is expensive