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State two features that must be visible in a 2-D diagram of a metallic lattice?
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regularly arranged positive metal ions; delocalised electrons shown between the ions / throughout the structure
Define metallic bonding?
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the strong electrostatic attraction; between positive metal ions and delocalised electrons
Explain why metallic bonding is described as a giant structure?
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the electrostatic attraction acts between all positive ions and all delocalised electrons throughout the structure; so millions of ions are bonded together in a continuous lattice
Explain why metals are good conductors of electricity?
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metals contain delocalised electrons; which are free to move through the structure, carrying electrical charge / forming a current
Explain why metals are malleable?
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layers of positive metal ions can slide over each other when a force is applied; the delocalised electrons shift with the ions; so the electrostatic attraction between positive ions and delocalised electrons is maintained in the new positions
Compare the electrical conductivity of a metal with that of a solid ionic compound, and explain the difference?
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metals conduct electricity but solid ionic compounds do not; metals have delocalised electrons that are free to move and carry charge; in solid ionic compounds, the ions are held in fixed positions and cannot move to carry charge