Chemistry might seem complicated, but understanding how metals behave is... Show more
Chemistry212 views·Updated May 18, 2026·3 pagesUnderstanding Reactivity in Chemistry
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1
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Metal Reactivity Basics
Ever wonder why some metals rust quickly whilst others stay shiny for years? It all comes down to reactivity - how eager metals are to lose electrons and form compounds.
Oxidation happens when metals gain oxygen or lose electrons. Think of it as metals "giving away" their electrons because they're generous like that. The more reactive a metal is, the more easily this happens.
Reduction is the opposite - it's when substances lose oxygen or gain electrons. Remember it as metals being "reduced" in their eagerness to react.
Quick Tip: Use the phrase "OIL RIG" - Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons)!
2
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The Reactivity Series and Displacement
The reactivity series is like a league table for metals, ranking them from most to least reactive. At the top, you've got potassium and sodium (seriously reactive), whilst gold and platinum chill at the bottom being practically unreactive.
Here's the order you need to know: Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Zinc, Iron, Copper, Silver, Gold, Platinum. The higher up the list, the more likely that metal is to lose electrons and form positive ions.
Displacement reactions happen when a more reactive metal kicks out a less reactive one from a compound. For example, magnesium can displace copper from copper sulfate because magnesium is higher in the reactivity series. It's like a stronger player taking someone else's position on the team.
Memory Trick: "Please Stop Lithium Calling My Aunt Zelda In Copper Silver Gloves Please" - use this to remember the reactivity series order!
3
of 3
Acids and Neutralisation
When metals meet acids, they create a salt plus hydrogen gas - it's one of the most predictable reactions in chemistry. This is also a redox reaction because the metal gets oxidised whilst the acid gets reduced.
Neutralisation happens when acids react with bases (anything with a pH above 7). You'll encounter three main types of bases: metal carbonates, metal oxides, and metal hydroxides. Each creates a slightly different reaction pattern.
Metal carbonates give you salt + water + carbon dioxide. Metal hydroxides produce salt + water. Metal oxides also create salt + water. The key is recognising which type of base you're dealing with, then you can predict the products every time.
Exam Tip: Always check if carbon dioxide is produced - it's the telltale sign you're dealing with a carbonate reaction!
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Chemistry212 views·Updated May 18, 2026·3 pagesUnderstanding Reactivity in Chemistry
hannah@hannah.revise
Chemistry might seem complicated, but understanding how metals behave is actually quite straightforward once you know the patterns. Let's break down metal reactivity, displacement reactions, and how metals interact with acids - concepts that'll pop up regularly in your GCSE... Show more
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Metal Reactivity Basics
Ever wonder why some metals rust quickly whilst others stay shiny for years? It all comes down to reactivity - how eager metals are to lose electrons and form compounds.
Oxidation happens when metals gain oxygen or lose electrons. Think of it as metals "giving away" their electrons because they're generous like that. The more reactive a metal is, the more easily this happens.
Reduction is the opposite - it's when substances lose oxygen or gain electrons. Remember it as metals being "reduced" in their eagerness to react.
Quick Tip: Use the phrase "OIL RIG" - Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons)!
2
of 3Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
The Reactivity Series and Displacement
The reactivity series is like a league table for metals, ranking them from most to least reactive. At the top, you've got potassium and sodium (seriously reactive), whilst gold and platinum chill at the bottom being practically unreactive.
Here's the order you need to know: Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Zinc, Iron, Copper, Silver, Gold, Platinum. The higher up the list, the more likely that metal is to lose electrons and form positive ions.
Displacement reactions happen when a more reactive metal kicks out a less reactive one from a compound. For example, magnesium can displace copper from copper sulfate because magnesium is higher in the reactivity series. It's like a stronger player taking someone else's position on the team.
Memory Trick: "Please Stop Lithium Calling My Aunt Zelda In Copper Silver Gloves Please" - use this to remember the reactivity series order!
3
of 3Sign up to see the content. It's free!
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Acids and Neutralisation
When metals meet acids, they create a salt plus hydrogen gas - it's one of the most predictable reactions in chemistry. This is also a redox reaction because the metal gets oxidised whilst the acid gets reduced.
Neutralisation happens when acids react with bases (anything with a pH above 7). You'll encounter three main types of bases: metal carbonates, metal oxides, and metal hydroxides. Each creates a slightly different reaction pattern.
Metal carbonates give you salt + water + carbon dioxide. Metal hydroxides produce salt + water. Metal oxides also create salt + water. The key is recognising which type of base you're dealing with, then you can predict the products every time.
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