| Metal + Oxygen → | Metal Oxide |
| Magnesium + Oxygen → | Magnesium Oxide |
| Metal + Water → | Metal Hydroxide + Hydrogen |
| Sodium + Water → | Sodium Hydroxide + Hydrogen |
| Metal + Acid → | Metal Salt + Hydrogen |
| Zinc + Sulfuric Acid → | Zinc Sulfate + Hydrogen |
| What Salt is Produced from a metal reacting with hydrochloric acid? | Chloride Salt |
| What salt is produced from reacting a metal with sulfuric acid? | Sulfate Salt |
| What salt is produced from a metal reacting with nitric acid? | Nitrate Salt |
| Name the metals stored under oil | Potassium, Sodium, Lithium |
| What metals react with acid but not water | Any metals between aluminium and lead in the electrochemical series |
| Describe the test for hydrogen gas | Test hydrogen gas with a lighted splint and it will go pop. |
| What is a metal ore? | A rock containing a naturally occurring metal compound. |
| Name two metal compounds that decompose on heating to produce the metal | Silver oxide, mercury oxide |
| What oxides are extracted by heating with carbon? | Any oxides from zinc oxide to lead oxide in the electrochemical series |
| What metals are extracted from their oxides by electrolysis | Any from Lithium oxide to aluminium oxide in the electrochemical series. |
| Name the metal extracted in a blast furnace | Iron |
| What happens in a displacement reaction and what would you observe? | When metals higher up in the reactivity series displace those lower down from solution you see the metal changing colour in a displacement reaction. |
| Write a word equation for magnesium displacing zinc from zinc sulfate solution | Magnesium + Zinc Sulfate → Magnesium sulfate + Zinc |
| What metals could displace iron from solution? | Any metals above iron in the electrochemical series |
| What is corrosion | A chemical reaction in which the surface of a metal changes into a compound from an element. |
| What are the two conditions required for rusting? | Oxygen and water |
| Describe the test for rust | Ferroxyl indicator changes colour from yellow to blue in the presence of rust. |
| Give the definition of galvanising | Coating iron in zinc |
| Why does galvanising protect iron from rusting? | It stops air and water reaching the iron. If scratched it corrodes instead of the iron and provides sacrificial protection |
| What is meant by sacrificial protection? | Connecting a metal above iron in the electrochemical series to slow the corrosion of iron. The higher up metal is sacrificed to protect the iron. |
| What metals could be used to protect iron from rusting by providing sacrificial protection? | Any metal higher than iron in the electrochemical series, usually magnesium, aluminium or zinc. |
| Can potassium, sodium or lithium be used for sacrificial protection? | No, as they are far too reactive and unstable in air. |
| What metals react with water, acid and oxygen? | Lithium, Potassium, Sodium, Magnesium |
| What metals react with oxygen and acid only? | Aluminium, zinc, iron, nickel, tin, lead |
| What metals react with only oxygen? | Copper, silver, mercury |
| What metal is completely unreactive with water, oxygen and acid? | Gold |
| List the reactivity series in order | Lithium, potassium, sodium, magnesium, aluminium, zinc, iron, nickel, tin, lead, copper, silver, mercury, gold. |
