Properties of metals
Cambridge IGCSE Chemistry (0620) · Unit 9: Metals · 10 flashcards
Properties of metals is topic 9.1 in the Cambridge IGCSE Chemistry (0620) syllabus , positioned in Unit 9 — Metals , alongside Reactivity series, Extraction of metals and Uses of metals. In one line: Metallic bonding consists of positive ions in a sea of delocalized electrons. There is a strong attraction between these positive ions and the delocalized electrons, holding the metal atoms together.
This topic is examined in Paper 1 (multiple-choice) and Papers 3/4 (theory), plus Paper 5 or Paper 6 (practical / alternative to practical).
The deck below contains 10 flashcards — 3 definitions, 5 key concepts and 2 identification cards — covering the precise wording mark schemes reward. Use the 3 definition cards to lock down command-word answers (define, state), then move on to the concept and application cards to handle explain, describe and compare questions.
Describe metallic bonding in terms of structure and forces
Metallic bonding consists of positive ions in a sea of delocalized electrons. There is a strong attraction between these positive ions and the delocalized electrons, holding the metal atoms together.
What the Cambridge 0620 syllabus says
Official 2026-2028 specThese are the exact learning objectives Cambridge sets for this topic. Match the command word (Describe, Explain, State, etc.) in your answer to score full marks.
- Compare Compare the general physical properties of metals and non-metals, including: (a) thermal conductivity (b) electrical conductivity (c) malleability and ductility (d) melting points and boiling points
- Describe Describe the general chemical properties of metals, limited to their reactions with: (a) dilute acids (b) cold water and steam (c) oxygen
Describe metallic bonding in terms of structure and forces.
Metallic bonding consists of positive ions in a sea of delocalized electrons. There is a strong attraction between these positive ions and the delocalized electrons, holding the metal atoms together.
Explain why metals are good conductors of electricity.
Metals are good conductors because they have delocalized electrons that are mobile and can flow freely throughout the structure, carrying an electrical charge.
Explain why metals are good conductors of thermal energy.
Delocalized electrons can move quickly through the structure transferring kinetic energy. Vibrations of the positive metal ions also contribute to thermal conductivity.
Define malleability.
Malleability is the ability of a metal to be hammered or pressed into shape without breaking. This is because the layers of atoms can slide over each other without disrupting the metallic bond.
Define ductility.
Ductility is the ability of a metal to be drawn into wires. The layers of atoms can slide over each other without disrupting the metallic bond.
Compare the general melting and boiling points of metals to those of non-metals.
Metals generally have high melting and boiling points due to the strong electrostatic forces of attraction between the positive ions and the sea of delocalized electrons. Non-metals typically have lower melting and boiling points.
What type of product is formed when a metal reacts with an acid?
When a metal reacts with a dilute acid, a salt and hydrogen gas are produced.
What is the general reaction between a metal and oxygen?
A metal reacts with oxygen to form a metal oxide.
Describe the reaction of sodium with cold water.
Sodium reacts vigorously with cold water to produce sodium hydroxide and hydrogen gas. The reaction is exothermic and produces a large amount of heat. Equation: 2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g)
Describe the reaction of iron with steam.
Iron reacts with steam (hot water in gaseous form) to produce iron oxide and hydrogen gas. The reaction is slower than with cold water and requires high temperatures. Equation: 3Fe(s) + 4H2O(g) -> Fe3O4(s) + 4H2(g)
Key Questions: Properties of metals
Describe metallic bonding in terms of structure and forces.
Metallic bonding consists of positive ions in a sea of delocalized electrons. There is a strong attraction between these positive ions and the delocalized electrons, holding the metal atoms together.
Define malleability.
Malleability is the ability of a metal to be hammered or pressed into shape without breaking. This is because the layers of atoms can slide over each other without disrupting the metallic bond.
Define ductility.
Ductility is the ability of a metal to be drawn into wires. The layers of atoms can slide over each other without disrupting the metallic bond.
Tips to avoid common mistakes in Properties of metals
- ● Metals BELOW carbon in the reactivity series can be extracted from their oxides using carbon; metals ABOVE carbon need electrolysis.
- ● Consider both what a metal does and does not react with to gauge its reactivity.
- ● Learn common applications: aluminium is used where lightness and corrosion resistance are key, stainless steel for its strength and resistance to rust.
- ● Create a table summarizing the reactions of common metals (Ca, Mg, Zn, Fe, Cu) with water, steam, and dilute acids, linking it to the metal reactivity series.
- ● Relate metal extraction method to reactivity: electrolysis (most reactive), carbon reduction (intermediate), native state (least reactive).
More topics in Unit 9 — Metals
Properties of metals sits alongside these Chemistry decks in the same syllabus unit. Each uses the same spaced-repetition system, so progress in one informs the next.
Cambridge syllabus keywords to use in your answers
These are the official Cambridge 0620 terms tagged to this section. Mark schemes credit responses that use the exact term — weave them into your answers verbatim rather than paraphrasing.
Key terms covered in this Properties of metals deck
Every term below is defined in the flashcards above. Use the list as a quick recall test before your exam — if you can't define one of these in your own words, flip back to that card.
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