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The photograph shows the Atomium in Brussels - Leaving Cert Chemistry - Question B - 2020
Question B
The photograph shows the Atomium in Brussels. The Atomium represents the crystal structure of iron magnified about 165 billion times. Each of the nine spheres, which... show full transcript
Worked Solution & Example Answer:The photograph shows the Atomium in Brussels - Leaving Cert Chemistry - Question B - 2020
Step 1
What is meant by corrosion of a metal?
Answer
Corrosion of a metal refers to the oxidation process that occurs when the surface of the metal reacts with the environment, such as air, moisture, or other corrosive agents. This process typically results in the deterioration and eventual return of the metal to its ore state, often observed as rust formation in iron.
Step 2
Compare the abilities of pure iron and pure aluminium to resist corrosion.
Answer
Pure aluminium is generally more resistant to corrosion than pure iron. This is because aluminium forms a protective oxide layer that adheres strongly to its surface, preventing further oxidation. In contrast, iron corrodes more easily and loses its protective oxide layer, leading to flaking and more rapid deterioration.
Step 3
What is the difference between iron and steel?
Answer
The primary difference between iron and steel is that steel is an alloy containing iron and carbon, along with other elements. While pure iron is malleable but can be relatively soft, steel gains additional strength and hardness due to the presence of carbon and other alloying elements, making it more suitable for a variety of structural applications.
Step 4
What is meant by anodising aluminium?
Answer
Anodising aluminium is a process that involves creating a thicker layer of aluminium oxide (Al₂O₃) on the surface of the aluminium. This is achieved through electrolysis, where the aluminium acts as the anode in an electrolyte solution. The anodised layer enhances corrosion resistance and allows for better dyeing and finishing.
Step 5
Why can metals conduct electricity?
Answer
Metals can conduct electricity due to the presence of free-moving valence electrons. These electrons are delocalized, meaning they can move freely between atoms, allowing for the efficient transmission of electric current throughout the metallic structure. This property makes metals excellent conductors of electricity.