Chemistry · Bonding, Structure and Properties of Matter
Properties of Metals and Alloys
Spec 5.2.2.7–5.2.2.8📙 Higher
Interactive · apply a force to pure metal vs alloy
Theory · read, then commit
Metals have giant metallic structures — a regular lattice of positive metal ions surrounded by a sea of delocalised electrons. That structure explains all their properties.
Properties of metals
🌡️High melting & boiling point
Strong forces between the positive ions and the electron sea (exceptions: mercury and gallium are liquid near room temperature).
🔨Malleable & ductile
Layers of ions slide and the electron sea re-accommodates them — so metals hammer into shape and draw into wires.
⚡Conducts electricity & heat (as a solid)
Delocalised electrons are free to move even in the solid, carrying both charge and thermal energy.
⚖️High density
A close-packed lattice of heavy atoms makes most metals dense.
Checkpoint · quick check
Explain why metals are good conductors of heat.
🏗️Key alloys and their uses
Steel (iron + carbon) — much harder than iron → construction, tools, vehicles.
Aluminium alloys — strong and lightweight → aircraft, spacecraft.
Checkpoint · quick check
Describe the difference in structure between a pure metal and one of its alloys.
⚠️ Common Mistake
Students often think that because ionic compounds only conduct when molten, metals must be the same. They are not: a metal conducts in the solid state because its delocalised electrons are already free to move. Ionic compounds cannot conduct as solids because their charge carriers are ions, which stay locked in place until the compound melts or dissolves.
Retrieval · Metal or Alloy — Property Match
Test yourself · 8 questions, exam order
⭐Examiner Tip
Two easy marks to lose: metals conduct as solids because their delocalised electrons are already free to move — don't say they must melt first like ionic compounds; and alloys are harder because different-sized atoms distort the layers so they can't slide. Name the delocalised electrons and the disrupted layers explicitly.
0 of 8 answered
Warm-up · 2 questions
Explain why metals can conduct electricity in the solid state, but ionic compounds cannot.
Explain why brass (copper mixed with zinc) is harder than pure copper.
Exam standard · 4 questions
Explain why pure metals are often too soft for use, so alloys are made instead.
Explain, in terms of particles, why metals conduct electricity and heat but simple molecular substances do not.
Stainless steel is used to make cutlery. Suggest two properties that make it suitable and relate them to its structure.
Explain why an alloy is generally harder than the pure metal it is made from, using the idea of layers of atoms.
Stretch · 2 questions
Aluminium is used for aircraft bodies. Suggest why an aluminium alloy is used rather than pure aluminium.
Explain why metals are malleable but ionic compounds are brittle, in terms of what happens when the layers move.
Key note · cover it, say it, check it
Revision card · 5 stepsProperties of Metals and Alloys