The reactivity series helps us understand how readily different metals...
Chemistry246 views·Updated 4 Aug 2026·3 pagesChemistry Basics: Metal Reactivity and Extraction
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The Reactivity of Metals
Metals vary greatly in their reactivity levels. The most reactive metals are found in Groups 1, 2 and 3 of the periodic table, including potassium, sodium, calcium and aluminium. Transition metals like iron, copper and zinc have medium reactivity, while gold, silver and platinum are notably unreactive.
When metals react with oxygen, they form metal oxides through a process called oxidation. The chemical equation follows the pattern: Metal + oxygen → metal oxide. For example, magnesium burns brightly in oxygen to form magnesium oxide (2Mg + O₂ → 2MgO).
Group 1 metals like potassium, sodium and lithium react extremely vigorously with oxygen even at room temperature. Medium-reactive metals like magnesium, zinc and iron react more slowly or require heating. The least reactive metals like gold and platinum don't react with oxygen at all.
Remember: The more reactive a metal is, the more vigorously it reacts with oxygen. Group 1 metals can be dangerous to handle because they react so readily with both oxygen and water!
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Reactions with Water and Acids
Reactive metals can displace hydrogen from water through the reaction: Metal + water → metal hydroxide + hydrogen. The highly reactive metals potassium, sodium and lithium react immediately with cold water, producing hydrogen bubbles. Potassium even burns with a distinctive purple flame during this reaction!
When metals react with acids, they follow the pattern: Metal + acid → metal salt + hydrogen. You'll observe bubbling as hydrogen gas is released, and the metal will gradually dissolve. Extremely reactive metals (potassium, sodium, lithium) react violently with acids, while calcium, magnesium, zinc and iron react steadily.
Displacement reactions occur when a more reactive metal takes the place of a less reactive metal in a compound. For example, when zinc is added to copper sulphate solution, zinc displaces copper because it's more reactive. You'll observe the blue solution becoming colourless as zinc sulphate forms, while solid copper appears as a brown deposit.
Quick tip: In displacement reactions, remember OIL RIG - Oxidation Is Loss of electrons, Reduction Is Gain of electrons. The more reactive metal loses electrons (oxidised) while the less reactive metal gains electrons (reduced).
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Extraction of Metals
How we extract metals from their ores depends entirely on the metal's reactivity. If a metal is less reactive than carbon, we can extract it using reduction with carbon. This method won't work for highly reactive metals.
In reduction with carbon, the metal oxide reacts with carbon to produce the pure metal and carbon dioxide. For example: Copper oxide + carbon → copper + carbon dioxide (2CuO + C → 2Cu + CO₂). During this process, copper oxide is reduced (it loses oxygen), while carbon is oxidised (it gains oxygen).
Looking at the electron transfer helps us understand what's happening. Copper starts as a 2+ ion (Cu²⁺) and ends with no charge (Cu), meaning it has gained electrons. Carbon loses electrons as it changes from an element to a compound, becoming oxidised.
Important concept: For metals more reactive than carbon (like aluminium, calcium and sodium), we must use electrolysis instead of carbon reduction. This requires more energy, making these metals more expensive to extract.
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Chemistry246 views·Updated 4 Aug 2026·3 pagesChemistry Basics: Metal Reactivity and Extraction
The reactivity series helps us understand how readily different metals react with substances like oxygen, water, and acids. This determines which metals can displace others in reactions and impacts how we extract metals from their ores. Let's explore how metals...
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The Reactivity of Metals
Metals vary greatly in their reactivity levels. The most reactive metals are found in Groups 1, 2 and 3 of the periodic table, including potassium, sodium, calcium and aluminium. Transition metals like iron, copper and zinc have medium reactivity, while gold, silver and platinum are notably unreactive.
When metals react with oxygen, they form metal oxides through a process called oxidation. The chemical equation follows the pattern: Metal + oxygen → metal oxide. For example, magnesium burns brightly in oxygen to form magnesium oxide (2Mg + O₂ → 2MgO).
Group 1 metals like potassium, sodium and lithium react extremely vigorously with oxygen even at room temperature. Medium-reactive metals like magnesium, zinc and iron react more slowly or require heating. The least reactive metals like gold and platinum don't react with oxygen at all.
Remember: The more reactive a metal is, the more vigorously it reacts with oxygen. Group 1 metals can be dangerous to handle because they react so readily with both oxygen and water!
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Reactions with Water and Acids
Reactive metals can displace hydrogen from water through the reaction: Metal + water → metal hydroxide + hydrogen. The highly reactive metals potassium, sodium and lithium react immediately with cold water, producing hydrogen bubbles. Potassium even burns with a distinctive purple flame during this reaction!
When metals react with acids, they follow the pattern: Metal + acid → metal salt + hydrogen. You'll observe bubbling as hydrogen gas is released, and the metal will gradually dissolve. Extremely reactive metals (potassium, sodium, lithium) react violently with acids, while calcium, magnesium, zinc and iron react steadily.
Displacement reactions occur when a more reactive metal takes the place of a less reactive metal in a compound. For example, when zinc is added to copper sulphate solution, zinc displaces copper because it's more reactive. You'll observe the blue solution becoming colourless as zinc sulphate forms, while solid copper appears as a brown deposit.
Quick tip: In displacement reactions, remember OIL RIG - Oxidation Is Loss of electrons, Reduction Is Gain of electrons. The more reactive metal loses electrons (oxidised) while the less reactive metal gains electrons (reduced).
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Extraction of Metals
How we extract metals from their ores depends entirely on the metal's reactivity. If a metal is less reactive than carbon, we can extract it using reduction with carbon. This method won't work for highly reactive metals.
In reduction with carbon, the metal oxide reacts with carbon to produce the pure metal and carbon dioxide. For example: Copper oxide + carbon → copper + carbon dioxide (2CuO + C → 2Cu + CO₂). During this process, copper oxide is reduced (it loses oxygen), while carbon is oxidised (it gains oxygen).
Looking at the electron transfer helps us understand what's happening. Copper starts as a 2+ ion (Cu²⁺) and ends with no charge (Cu), meaning it has gained electrons. Carbon loses electrons as it changes from an element to a compound, becoming oxidised.
Important concept: For metals more reactive than carbon (like aluminium, calcium and sodium), we must use electrolysis instead of carbon reduction. This requires more energy, making these metals more expensive to extract.
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