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9.1Metals

Properties of metals — Combined Science 0653 - Chemistry Revision Notes & Topical Questions

5 min read 9 parts Lesson 2 of 11 1 quiz

📚 Combined Science 0653 - Chemistry Hub / Topical Revision
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Lesson summary

9.1 Properties of metals — COMBINED SCIENCE (CHEMISTRY) notes: Compare the physical and chemical properties of metals and non-metals.Elements — most elements are metals and a few, metalloids, show properties of both.Trend — metallic character decreases from left to right across t…

  • Cold water
  • Reactivity
  • Delocalised electrons
  • Metallic bond
  • Trend — metallic character decreases from left to right across the Periodic Table
  • Steam — some metals form a metal oxide and hydrogen.Zn + H2O → ZnO + H2

Section 1 of 9Metals and non-metals

Elements
  • Elements most elements are metals and a few, metalloids, show properties of both.
Trend
  • Trend metallic character decreases from left to right across the Periodic Table.

Section 2 of 9Physical properties of metals

PropertyExplanation
Conduct heat and electricityDelocalised electrons move through the structure
Malleable and ductileLayers of positive ions slide over each other
High melting and boiling pointsStrong attraction between positive ions and delocalised electrons needs much energy to break

Section 3 of 9Physical properties of non-metals

PropertyExplanation
Do not conduct heat and electricityAll electrons are in covalent bonds (graphite is an exception)
Brittle when solidNot malleable or ductile
Low melting and boiling pointsWeak forces between molecules; many are gases (diamond and silicon(IV) oxide are exceptions)

Section 4 of 9Reaction with water

Cold water
  • Cold water some metals form a metal hydroxide and hydrogen.
  • Ca + 2H2O → Ca(OH)2 + H2.
Steam
  • Steam some metals form a metal oxide and hydrogen.
  • Zn + H2O → ZnO + H2.

Section 5 of 9Reaction with acids

Equation
  • Equation metal + acid → salt + hydrogen.
  • Fe + 2HCl → FeCl2 + H2.
Reactivity
  • Reactivity most metals react with acids, with more reactive metals reacting more vigorously.

Section 6 of 9Reaction with oxygen

Equation
  • Equation metal + oxygen → metal oxide.
  • 2Cu + O2 → 2CuO.
Reactivity
  • Reactivity gold and platinum do not react, alkali metals react easily, and copper and iron react slowly.

Section 7 of 9More from the specification

More from the specification
Metallic bonding and structure
  • Positive metal ions arranged in regular close-packed layers surrounded by a sea of delocalised electrons.
Alloys structure
  • Mixtures of a metal with other elements containing different sized atoms that distort regular layers, preventing them from sliding easily.
Aluminium properties
  • Low density, high thermal conductivity, and excellent corrosion resistance due to a self-healing surface oxide layer (Al2O3).
Corrosion resistance
  • Protective oxide films prevent atmospheric oxygen and moisture from attacking inner reactive metal layers.
Alloy
  • A mixture of a metal with one or more other elements.
Corrosion
  • The gradual destruction of a metal by reaction with its surroundings.
Density
  • Mass divided by volume.

Section 8 of 9Key terms

TermMeaning
Delocalised electronsElectrons free to move through a metal.
MalleableCan be hammered into shape.
DuctileCan be drawn into wires.
MetalloidElement with properties of metals and non-metals.
Metallic bondAttraction between positive ions and delocalised electrons.

Section 9 of 9Exam technique

1
Saying metals conduct because of free ions — delocalised electrons carry charge.
2
Saying all non-metals are poor conductors — graphite conducts.
3
Saying metals are brittle — they are malleable.
4
Saying all metals react with water.

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