Structure & Properties of Giant Lattices — GCSE Chemistry Revision
Revise Structure & Properties of Giant Lattices for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
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Go to Diamond, Graphite & GrapheneWhat is Structure & Properties of Giant Lattices?
Giant lattice structures are found in ionic compounds, covalent network solids (like diamond), and metals. They consist of a huge, repeating three-dimensional arrangement of particles, resulting in high melting points and specific physical properties.
Board notes: This topic is fundamental and links bonding to properties. All boards expect you to be able to relate the structure of giant lattices (ionic, metallic, and giant covalent) to their physical properties like melting point, conductivity, and hardness.
Step-by-step explanationWorked example
Sodium chloride (NaCl) forms a giant ionic lattice. Each Na⁺ ion is surrounded by six Cl⁻ ions, and each Cl⁻ ion is surrounded by six Na⁺ ions. This strong, repeating pattern makes salt crystals hard and gives them a high melting point (801°C).
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Common mistakes
- 1Thinking all covalent substances have low melting points. Giant covalent structures like diamond and silica have very high melting points.
- 2Confusing the structure of graphite with other giant lattices. Graphite has layers that can slide, which is unusual for a giant structure.
- 3Forgetting that the formula of an ionic compound represents the ratio of ions in the lattice, not a single molecule.
Structure & Properties of Giant Lattices exam questions
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Structure & Properties of Giant Lattices
Core concept
Giant lattice structures are found in ionic compounds, covalent network solids (like diamond), and metals. They consist of a huge, repeating three-dimensional arrangement of particles, resulting in hi…
Frequently asked questions
Why is diamond so hard?
In diamond, each carbon atom is joined to four other carbon atoms by strong covalent bonds. This creates a rigid, tetrahedral network structure that is very difficult to break, making diamond extremely hard.
What is a unit cell?
A unit cell is the smallest repeating unit of a crystal lattice. The entire crystal can be built up by repeating the unit cell in three dimensions.