Flashcards
Mettalic Bonding
Cards in this deck (8)
- 1Define metallic bondingThe electrostatic attraction between positive ions and a sea of delocalised electrons
- 2Describe how metallic bonding takes placeThe outermost electrons of a metal atom are delocalised. This leaves a positive metal cation (e.g. Na⁺, Mg²⁺, Al³⁺)
- 3Name the structure in which metal elements existGiant metallic lattice structures
- 4Describe the properties of giant metallic lattice structuresMalleable 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 - 5Why are metals malleable and ductile?No bonds hold specific ions together - metal ions can slide over each other when the structure is pulled
- 6Why are metals good thermal/electrical conductor?THERMAL
Delocalised electrons can pass kinetic energy
ELECTRICAL
Delocalised electrons can carry a current - 7What 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
- 8TRUE OR FALSE: The size of the metal ion and lattice structure affects melting/boiling pointTRUE
A smaller ionic radius will hold the delocalised electrons closer to the nuclei
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- User has deleted their subject information Flashcards on Mettalic Bonding, created by Deleted user on 05/03/2018.
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- Deleted user · Mar 2018
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- Mar 5, 2018
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- Created by Yinka F · Mar 3, 2018
- Copied by Yinka F · Mar 5, 2018
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