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5 - Structure and Bonding

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  • ✓Describe and explain chemical bonding in terms of the behaviour of electrons.
  • ✓Distinguish between ionic, covalent, and metallic bonding.
  • ✓Illustrate bond formation using dot-and-cross diagrams.
  • ✓Write correct chemical formulae of ionic compounds.
  • ✓Explain how the structure of solids affects their physical properties.
  • ✓Compare the properties of ionic, covalent, and metallic substances.
  • ✓Explain the structure and properties of diamond and graphite.
  • ✓Define and give examples of allotropy.
⏱ 0 mins🎯 43 marks
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Why does sodium metal react explosively with water but neon gas doesn’t? The answer lies in stability, all atoms want to achieve a full outer shell of electrons (like the noble gases). Atoms combine through chemical bonding to become stable, forming compounds with new properties.
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💡EngageQuestion 11 of 27

Predict: which statement do you think best describes an atom?

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Always show electron transfer or sharing using dot-and-cross diagrams. Use valency to derive correct ionic formulae. Compare properties, melting point, conductivity, solubility. Know diamond vs graphite structures for Paper 02 questions. Atoms bond to achieve stability (full outer shell). Ionic bonds → transfer of electrons; between metals & non-metals; strong electrostatic forces. Covalent bonds → sharing of electrons; between non-metals; weak intermolecular forces. Metallic bonds → lattice of positive ions in sea of electrons; explain conductivity. Structure affects properties, strong bonds = high melting points; delocalised electrons = conductivity. Carbon allotropes: Diamond = hard, non-conductor; Graphite = soft, conductor.
💡Engage
Why does sodium metal react explosively with water but neon gas doesn’t? The answer lies in stability, all atoms want to achieve a full outer shell of electrons (like the noble gases). Atoms combine through chemical bonding to become stable, forming compounds with new properties.
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