What are the general properties of metals according to the Cambridge IGCSE Chemistry syllabus?

Metals generally have high melting and boiling points, are good conductors of heat and electricity, are malleable and ductile, and have a shiny appearance. They tend to lose electrons easily, forming positive ions. These properties are emphasized in the Cambridge IGCSE Chemistry curriculum.

Why are metals good conductors of electricity?

Metals are good conductors of electricity because they have free electrons that can move easily throughout the metal lattice. This movement of electrons allows electrical current to pass through the metal efficiently, a concept covered in the Cambridge IGCSE Chemistry syllabus.

How does the malleability of metals benefit their use in everyday applications?

The malleability of metals, which allows them to be hammered or rolled into thin sheets without breaking, makes them ideal for a wide range of applications, such as in the manufacturing of car bodies, foil, and various household items. This property is crucial for understanding the practical uses of metals in the Cambridge IGCSE Chemistry course.

What is the significance of alloys in modifying the properties of metals?

Alloys are mixtures of metals with other elements that enhance certain properties, such as strength, corrosion resistance, or ductility. For example, adding carbon to iron creates steel, which is stronger and more durable. The study of alloys and their properties is an important part of the Cambridge IGCSE Chemistry syllabus.

How does the reactivity of metals vary across the periodic table?

The reactivity of metals generally increases as you move down a group in the periodic table and decreases across a period from left to right. This trend is due to the ease with which metals can lose electrons to form positive ions. Understanding these trends is essential for Cambridge IGCSE Chemistry students studying the properties of metals.

Why is "Calling an alloy a compound" a common mistake in Properties of Metals?

Why it happens: Two elements combined. How to avoid it: Alloy = MIXTURE (variable proportions, no chemical bond change). Source: 0620/42 — recurring

Why is "Saying metals conduct because of 'mobile particles'" a common mistake in Properties of Metals?

Why it happens: Imprecise language. How to avoid it: Conduction is due to DELOCALISED electrons.

Why is "Saying ALL metals have high density" a common mistake in Properties of Metals?

Why it happens: Generalising. How to avoid it: MOST metals have high density. Exceptions exist (Li, Na float on water).

MetalsCambridge IGCSE Chemistry (0620)

Properties of Metals

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Properties of Metals — Cambridge IGCSE 0620 Chemistry Extended (2026)

Physical and chemical properties of metals, plus alloys. Why metals conduct, why they're malleable, why alloys are harder.

What you’ll learn

Mapped to the Cambridge IGCSE 0620 syllabus (2026-2028).

11.1 — Describe the physical properties of metals.
11.1 — Describe the general chemical reactions of metals (with O₂, water, acids).
11.1 — Describe alloys and explain why they are harder than pure metals.

Physical properties of metals

Shiny, malleable/ductile, good conductors. All explained by metallic bonding (sea of electrons).

Standard properties.

Shiny / lustrous — delocalised electrons reflect light.
Malleable — can be hammered into shape.
Ductile — can be drawn into wires.
Good thermal conductors — delocalised electrons transfer heat.
Good electrical conductors — delocalised electrons carry charge.
High m.p. and density (mostly).
Sonorous — ring when struck.

All explained by the metallic bond. Positive metal ions in a sea of delocalised electrons (see Metallic Bonding study note).

Conductivity: electrons free to move.
Malleability/ductility: layers of ions slide; sea of electrons keeps the bonding.
High m.p.: strong electrostatic attraction across the whole lattice.

Exceptions to remember.

Mercury: only metal liquid at room temperature.
Sodium, potassium: very low m.p., easily cut with knife.
Lithium: less dense than water (floats).

Cambridge tip. When asked "explain why metals conduct", mention BOTH the existence of delocalised electrons AND their free movement.

Shiny, malleable, ductile, conductive (heat and electricity), high m.p.
All from metallic bonding.
Mercury: liquid at room T.
Group 1: low density, low m.p.

Chemical reactions of metals

Metals + O₂ → metal oxides. Metals + water → hydroxide + H₂. Metals + acid → salt + H₂.

1. With oxygen. $\text{metal} + \text{O}_{2} \to \text{metal oxide}.$

Reactive metals burn brilliantly: Mg burns with WHITE flame → MgO (white powder).
Less reactive metals oxidise slowly: Cu in air at room T forms a thin black CuO layer over time.
Most metal oxides are BASIC (react with acids); a few (Al, Zn) are AMPHOTERIC.

2. With water (or steam).

Group 1 metals: vigorous with cold water → metal hydroxide + H₂.
Mg: slow with cold water; vigorous with steam → MgO + H₂.
Zn, Fe: react with steam → metal oxide + H₂.
Cu and below: don't react with water (don't rust).

$2\text{Na} + 2\text{H}_{2}\text{O} \to 2\text{NaOH} + \text{H}_{2}.$

3. With dilute acid. $\text{metal} + \text{acid} \to \text{salt} + \text{hydrogen}.$

All metals ABOVE hydrogen in the reactivity series react.
Cu and below DO NOT react.

$\text{Mg} + 2\text{HCl} \to \text{MgCl}_{2} + \text{H}_{2}.$

Vigour follows the reactivity series. K reacts most vigorously, even Mg fizzes briskly. Zn fizzes slowly. Fe slow. Cu - none.

Worked qualitative. Why doesn't gold tarnish or react in normal conditions? Gold is below H in the reactivity series; doesn't react with O₂, water, or dilute acid at room temperature.

- O₂ → metal oxide (basic, mostly).
- water (or steam) → hydroxide / oxide + H₂.
- acid → salt + H₂.
Vigour follows reactivity series.

Alloys

Mixture of a metal with another element. Harder than the pure metal because layers can't slide.

Alloy. A mixture of a metal with one or more other elements (often other metals).

Why mix? Pure metals are often too soft for engineering. Alloys are harder, stronger, often more corrosion-resistant.

Why are alloys harder? Different-sized atoms in the lattice DISRUPT the regular layer arrangement. The smaller atoms (e.g. carbon in steel) sit in spaces between larger metal atoms, preventing layers from sliding past each other.

Common alloys.

Alloy	Composition	Use
Brass	Cu + Zn	Musical instruments, fittings, screws
Bronze	Cu + Sn	Statues, bells, bearings
Steel	Fe + C (and others)	Construction, vehicles, tools
Stainless steel	Fe + Cr + Ni	Kitchen utensils, medical instruments
Solder	Sn + Pb (older) or Sn + Cu	Joining electronics
Pewter	Sn + Cu + Bi	Decorative items
Duralumin	Al + Cu + Mg + Mn	Aircraft (light + strong)

Stainless steel. Adding chromium creates a thin invisible Cr₂O₃ layer that protects underlying iron from rusting. Adding nickel improves toughness.

Worked qualitative. Why is brass used for door handles instead of pure copper? Brass is harder (zinc atoms disrupt copper's lattice), more wear-resistant, and tarnishes less.

Alloy = metal + other element(s).
Harder than pure metal.
Different-sized atoms block layer sliding.
Common: brass, bronze, steel, stainless steel.

How it’s examined

Properties of metals appears every Paper 2 (3-4 marks: list properties, explain conductivity) and Paper 4 (4-6 marks: alloy hardness, predict reaction product). Examiner reports flag students explaining alloy hardness as just 'mixed metals are stronger' — Cambridge wants the layer-sliding explanation.

Sources: Cambridge IGCSE Chemistry 0620 syllabus 2026-2028 (11.1); 0620/22 May/Jun 2024 — Q13 (alloys, properties); 0620 Examiner Reports 2022-2024. Last reviewed 2026-05-07.

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Step-by-step worked examples — Properties of Metals

Step-by-step solutions to past-paper-style questions on properties of metals, written exactly the way a tutor would explain them at the board.

1Physical properties of metals
Core• physical
Question
State four physical properties typical of metals.
Step-by-step solution
1. Step 1
  (a) Good conductors of heat and electricity.
2. Step 2
  (b) Malleable and ductile.
3. Step 3
  (c) Shiny when polished (lustrous).
4. Step 4
  (d) High density and high melting/boiling points (most).
Answer
Good conductors, malleable/ductile, lustrous, high density and m.p.
2Why alloys are stronger than pure metals
Extended• Adapted from 0620/42 May/Jun 2024 Q12• alloys
Question
Explain why brass is harder than pure copper.
Step-by-step solution
1. Step 1
  In a pure metal, layers of identical-size atoms slide easily.
2. Step 2
  An alloy has different-sized atoms (Cu and Zn) that distort the layers.
3. Step 3
  Layers can no longer slide easily → harder, less malleable.
Answer
Different-sized atoms in an alloy disrupt the regular layers, preventing easy sliding.
3React with water
Extended• water
Question
Compare how Na, Ca and Mg react with cold water.
Step-by-step solution
1. Step 1
  Na: reacts vigorously with cold water → NaOH + H₂.
2. Step 2
  Ca: reacts steadily with cold water → Ca(OH)₂ + H₂.
3. Step 3
  Mg: very slow with cold water; faster with steam → MgO + H₂.
Answer
Reactivity decreases: Na > Ca > Mg. Different products with cold water vs steam.

Key Definitions and Keywords — Properties of Metals

Definitions to memorise and the exact keywords mark schemes credit for properties of metals answers — sharpened from recent examiner reports for the 2026 0620 sitting.

Malleable
Examiner keyword
Can be hammered or rolled into thin sheets without shattering.
Ductile
Examiner keyword
Can be drawn out into wires.
Alloy
Examiner keyword
A mixture of a metal with one or more other elements (often metals or carbon).
Lustrous
Shiny when freshly polished.

Common Mistakes and Misconceptions — Properties of Metals

The traps other students keep falling into on properties of metals questions — taken from recent Cambridge IGCSE 0620 examiner reports and mark schemes — and how to avoid them.

✕Calling an alloy a compound
0620/42 — recurring
Why it happens
Two elements combined.
How to avoid it
Alloy = MIXTURE (variable proportions, no chemical bond change).
✕Saying metals conduct because of 'mobile particles'
Why it happens
Imprecise language.
How to avoid it
Conduction is due to DELOCALISED electrons.
✕Saying ALL metals have high density
Why it happens
Generalising.
How to avoid it
MOST metals have high density. Exceptions exist (Li, Na float on water).

Practice questions

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Properties of Metals — frequently asked questions

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Properties of Metals

Short Study Notes in the form of Slides

Detailed Study Notes

What you’ll learn

How it’s examined

1Physical properties of metals

2Why alloys are stronger than pure metals

3React with water

Malleable

Ductile

Alloy

Lustrous

✕Calling an alloy a compound

✕Saying metals conduct because of 'mobile particles'

✕Saying ALL metals have high density

Practice questions

Past paper style quiz

Assess your understanding

Video lesson

Properties of Metals — frequently asked questions