Chemical changes are all around you - from the fizz...
Chemistry174 views·Updated Jun 14, 2026·2 pagesGCSE Chemistry C5 Notes: Triple Higher (Simplified)
Heidi@_heidi.1989.
1
of 2
Reactivity Series and Metal Extraction
Ever wondered why some metals rust whilst others stay shiny forever? The reactivity series ranks metals from most reactive (potassium) to least reactive (gold). This ranking tells you exactly how metals will behave in different situations.
Potassium, sodium, and lithium are so reactive they'll explode or fizz violently with water, creating alkaline metal hydroxide solutions and hydrogen gas. Metals like magnesium, aluminium, and zinc react more calmly with dilute acids, producing hydrogen gas and forming salts. Meanwhile, copper, silver, and gold are so unreactive they won't even react with steam.
Here's the clever bit: more reactive metals can displace less reactive ones from their salt solutions. This is why zinc can push copper out of copper sulphate solution. Remember oxidation is loss of electrons, reduction is gain of electrons - this happens in all these reactions.
When it comes to extracting metals from ores, the reactivity series determines the method. Unreactive metals like gold exist naturally, metals below carbon get reduced by carbon, and the most reactive metals need electrolysis to extract them.
Quick Tip: The reactivity series is like a league table - the higher up, the more likely a metal is to react and displace others below it.
2
of 2
Acids, Bases and Salt Formation
Making salts isn't just for chemistry labs - it's happening in your stomach when you take antacids and in factories making fertilisers. A salt forms when hydrogen in an acid gets replaced by metal or ammonium ions.
You can make salts using three key reactions: metal + acid → salt + hydrogen, acid + base → salt + water, and acid + carbonate → salt + carbon dioxide + water. The metal must be above hydrogen in the reactivity series to react with acids.
Strong acids like hydrochloric, nitric, and sulphuric acid completely break apart in water, giving low pH values. Weak acids like ethanoic acid (vinegar) and citric acid only partially ionise, so they have higher pH values and are reversible reactions.
When making salts from insoluble bases, you get neutralisation reactions where all charges balance to zero. You can get pure, dry salt crystals by evaporating the water and using indicators like litmus paper to check when the reaction is complete.
Remember: Strong acids are like bullies - they completely ionise and push all their H+ ions into solution. Weak acids are more polite and only release some of their hydrogen ions.
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Chemistry174 views·Updated Jun 14, 2026·2 pagesGCSE Chemistry C5 Notes: Triple Higher (Simplified)
Heidi@_heidi.1989.
Chemical changes are all around you - from the fizz when you drop a tablet in water to the rust on old bikes. Understanding how metals react and how to make different compounds is crucial for your GCSE chemistry success.
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Reactivity Series and Metal Extraction
Ever wondered why some metals rust whilst others stay shiny forever? The reactivity series ranks metals from most reactive (potassium) to least reactive (gold). This ranking tells you exactly how metals will behave in different situations.
Potassium, sodium, and lithium are so reactive they'll explode or fizz violently with water, creating alkaline metal hydroxide solutions and hydrogen gas. Metals like magnesium, aluminium, and zinc react more calmly with dilute acids, producing hydrogen gas and forming salts. Meanwhile, copper, silver, and gold are so unreactive they won't even react with steam.
Here's the clever bit: more reactive metals can displace less reactive ones from their salt solutions. This is why zinc can push copper out of copper sulphate solution. Remember oxidation is loss of electrons, reduction is gain of electrons - this happens in all these reactions.
When it comes to extracting metals from ores, the reactivity series determines the method. Unreactive metals like gold exist naturally, metals below carbon get reduced by carbon, and the most reactive metals need electrolysis to extract them.
Quick Tip: The reactivity series is like a league table - the higher up, the more likely a metal is to react and displace others below it.
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of 2Sign up to see the content. It's free!
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Acids, Bases and Salt Formation
Making salts isn't just for chemistry labs - it's happening in your stomach when you take antacids and in factories making fertilisers. A salt forms when hydrogen in an acid gets replaced by metal or ammonium ions.
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Strong acids like hydrochloric, nitric, and sulphuric acid completely break apart in water, giving low pH values. Weak acids like ethanoic acid (vinegar) and citric acid only partially ionise, so they have higher pH values and are reversible reactions.
When making salts from insoluble bases, you get neutralisation reactions where all charges balance to zero. You can get pure, dry salt crystals by evaporating the water and using indicators like litmus paper to check when the reaction is complete.
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