Bonding
- Created by: Shannon
- Created on: 05-03-14 17:35
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- Bonding
- Ionic
- Metal + non-metal
- Oppositely charged ions formed
- Held together by electrostatic forces of attraction
- Held in an arrangement known as a giant lattice structure
- This simple arrangement maximises the forces of attraction between ions - minimising repulsion
- Held in an arrangement known as a giant lattice structure
- Formed by either the loss (+ve ion) or gain (-ve ion) of electrons
- Held together by electrostatic forces of attraction
- Octet rule
- Ions form with a full outer shell of electrons
- Stability
- Ions form with a full outer shell of electrons
- Lattice energy
- The formation of one mole of an ionic compound from gaseous ions under standard conditions
- Affected by charge density
- As the size of the ion increased, the lattice energy becomes less negative
- In smaller ions, the cation is more polarising
- As the size of the ion increased, the lattice energy becomes less negative
- Values are compared using Born-Haber cycles
- Covalent
- Electron sharing
- In order to achieve full outer shell
- Most evident in elements in the middle of the periodic table
- Need to lose or gain several electrons - and this requires a lot of energy
- Balance between attractive and repulsive forces
- Electron density is shared
- Dative covalent bonding
- The electrons that make the bond come from the same atom
- Arises due to strong electrostatic forces of attraction between nucleus and the electrons
- Non-metal + non-metal
- Electron sharing
- Metallic
- Giant lattices of positive metal ions surrounded by a 'sea' of delocalised electrons
- Strong forces of attraction between metal ions and delocalised electrons
- Properties
- Electrical conductivity
- Delocalised electrons are free to move through the lattice
- Thermal conductivity
- Delocalised electrons can move easily, and so can transmit kinetic energy quickly through the lattice
- High melting and boiling point
- The strong attraction between the positive ions and negative electrons requires a lot of energy to separate
- Electrical conductivity
- Ionic
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