9.4

Uses of metals

10 flashcards to master Uses of metals

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Key Concept Flip

State the order of the reactivity series (most to least reactive).

Answer Flip

Potassium, sodium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold.

Key Concept Flip

What happens when potassium, sodium, and calcium react with cold water?

Answer Flip

Potassium, sodium, and calcium react vigorously with cold water, producing hydrogen gas and a metal hydroxide. Potassium reacts the most vigorously, followed by sodium and then calcium.

Example: 2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g)
Key Concept Flip

What happens when magnesium reacts with steam?

Answer Flip

Magnesium reacts with steam (H₂O in gaseous form) to produce magnesium oxide (MgO) and hydrogen gas (H₂).

Example: Mg(s) + H₂O(g) → MgO(s) + H₂(g)
Key Concept Flip

Which of these metals react with dilute hydrochloric acid: magnesium, zinc, iron, copper, silver, gold?

Answer Flip

Magnesium, zinc, and iron react with dilute hydrochloric acid to produce hydrogen gas and a metal chloride. Copper, silver, and gold do not react because they are below hydrogen in the reactivity series.

Example: Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)
Key Concept Flip

Explain why some metals react with dilute hydrochloric acid and others don't.

Answer Flip

Metals above hydrogen in the reactivity series can displace hydrogen ions (H⁺) from the acid to form hydrogen gas and a metal salt. Metals below hydrogen cannot displace the hydrogen ions.

Example: Iron can displace hydrogen, while copper can't.
Key Concept Flip

How can you deduce an order of reactivity from experimental results of metal reactions with acids?

Answer Flip

Observe the rate of reaction (

Example: speed of bubble formation, heat produced). A more vigorous reaction (faster bubble formation, more heat) indicates a more reactive metal. Comparing different metals reacting with the same acid can establish a relative order.
Key Concept Flip

Relate a metal's reactivity to its tendency to form positive ions.

Answer Flip

More reactive metals have a greater tendency to lose electrons and form positive ions (cations). This is why they readily react with other substances.

Example: Sodium easily forms Na⁺, making it very reactive.
Definition Flip

What is a displacement reaction involving aqueous ions?

Answer Flip

A displacement reaction is when a more reactive metal displaces a less reactive metal from its aqueous salt solution. For

Example: Iron will displace copper from copper sulfate solution: Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)
Key Concept Flip

Describe a displacement reaction between magnesium and copper(II) ions.

Answer Flip

Magnesium is more reactive than copper. When magnesium metal is added to a solution containing copper(II) ions (

Example: copper(II) sulfate), magnesium displaces the copper ions, forming magnesium ions and solid copper: Mg(s) + Cu²⁺(aq) → Mg²⁺(aq) + Cu(s)
Key Concept Flip

Explain why aluminium appears unreactive, even though it is high in the reactivity series.

Answer Flip

Aluminium readily reacts with oxygen in the air to form a thin, strong, and unreactive layer of aluminium oxide (Al₂O₃) on its surface. This oxide layer prevents further reaction with other substances, making aluminium appear unreactive.

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9.3 Extraction of metals 9.5 Corrosion

Key Questions: Uses of metals

What is a displacement reaction involving aqueous ions?

A displacement reaction is when a more reactive metal displaces a less reactive metal from its aqueous salt solution. For

Example: Iron will displace copper from copper sulfate solution: Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)

About Uses of metals (9.4)

These 10 flashcards cover everything you need to know about Uses of metals for your Cambridge IGCSE Chemistry (0620) exam. Each card is designed based on the official syllabus requirements.

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