Reactivity Series Flashcards
State the reactivity series.
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Hydrogen
Copper
Silver
Gold
What is a displacement reaction?
A reactions where a more reactive element takes the place of the less reactive element.
Describe the reaction between magnesium and magnesium sulfate
No reaction
Describe the reaction between magnesium sulfate and zinc
No reaction
Describe the reaction between magnesium sulfate and copper
No reaction
Describe the reaction between magnesium sulfate and iron
No reaction
Describe the reaction between zinc sulfate and magnesium
Grey solid to grey solid. Ribbon disappeared. Colourless solution to colourless solution.
Describe the reaction between zinc sulfate and zinc
No reaction
Describe the reaction between zinc sulfate and copper
No reaction
Describe the reaction between zinc sulfate and iron
No reaction
Describe the reaction between copper sulfate and magnesium
Solid grey to red brown. Blue solution to colourless
Describe the reaction between copper sulfate and zinc
Grey solid to red brown. Blue solution to colourless
Describe the reaction between copper sulfate and copper
No reaction
Describe the reaction between copper sulfate and iron
Grey solid to red brown. Blue solution to green
Describe the reaction between iron sulfate and magnesium
Grey solid to grey solid. Green solution to colourless.
Describe the reaction between iron sulfate and zinc
Grey solid to grey solid. Green solution to colourless.
Describe the reaction between iron sulfate and iron
No reaction
Describe the reaction between iron sulfate and copper
No reaction
Define oxidation
Gain of oxygen
Define redox
A reaction in which both oxidisation and reduction occur
Define reduction
Loss of oxygen
What is the chemical and word equation for the thermite reaction.
Aluminium + iron oxide —> iron + aluminium oxide
2Al + Fe(lll)2O3 —> 2Fe + Al2O3
Define ore
Contains metal compounds found in nature.
How can you obtain a pure metal from its oxide? (When it is less reactive than carbon)
You react the metal oxide with carbon, carbon displaces it, leaving the pure metal behind.
How can you extract a pure metal from its oxide? (When it is more reactive than carbon)
Electrolysis
Which metals are native, what does that mean?
Native is that it is already naturally pure, they are below copper in the reactivity series. Eg. Lead, silver, gold
What is the formula of rust
Fe2O3
In what conditions can iron rust?
Water and oxygen
Why is rust bad?
Iron and steel are strong and malleable, ionic compounds are brittle (rust) can no longer be used.
Note: steel is an allowed of iron and carbon.
How does physical barriers prevent rusting?
You cover the iron with something like paint to prevent water and oxygen from reaching the iron.
Pro and Con of physical barriers.
Pro = cheap
Con = worn away easily in things like railways.
How does galvanising prevent rusting?
When steel and iron are coated in molten zinc. Is a combination of both physical barriers and sacrificial protection.
How does sacrificial protection prevent rusting?
Covering the iron and steel with a more reactive metal. This means that the water and oxygen would react wit( the more reactive metal instead of the iron and steel.
Pros and cons of sacrificial protection.
Pro = prevents rusting effectively
Con = the more reactive metal gets used up quickly
