12595149
| Question | Answer |
| Define metallic bonding | The electrostatic attraction between positive ions and a sea of delocalised electrons |
| Describe how metallic bonding takes place | The outermost electrons of a metal atom are delocalised. This leaves a positive metal cation (e.g. Na⁺, Mg²⁺, Al³⁺) |
| Name the structure in which metal elements exist | Giant metallic lattice structures |
| Describe the properties of giant metallic lattice structures | Malleable and ductile (can be shaped/drawn into a wire) Good thermal and electrical conductor Insoluble (EXCEPT in liquid metals) Number of delocalised electrons per atom affects melting and boiling point |
| Why are metals malleable and ductile? | No bonds hold specific ions together - metal ions can slide over each other when the structure is pulled |
| Why are metals good thermal/electrical conductor? | THERMAL Delocalised electrons can pass kinetic energy ELECTRICAL Delocalised electrons can carry a current |
| What happens to the melting/boiling point as the number of delocalised electrons increase? | The more delocalised electrons there are, the stronger the bonding will be and the higher the melting/boiling point |
| TRUE OR FALSE: The size of the metal ion and lattice structure affects melting/boiling point | TRUE A smaller ionic radius will hold the delocalised electrons closer to the nuclei |
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