Metallic bonding
Cards (12)
- Properties of non-metals
- not shiny
- Low melting and boiling point
- Brittle
- metal properties:
- Sonorous
- Conduct electricity and heat
- Shiny when polished
- High melting and boiling point
- Delocalized electrons are free to move around the lattice and can be used to carry out chemical reactions. Explains why metals can conduct electricity and heat.
- Metalic bond is the electrostatic attraction between the delocalized electrons and the positive metal ions in the lattice
- Metal conducts electricity:
- Delocalized electrons in the metal structure can move an electric current flow because of the movement of electrons or charged particles.
- Delocalised electrons can carry the charge
- Metal can conduct heat:
- When particles can move and are close together to pass on the heat
- Delocalised electrons in the metal structure enable heat energy to be passed through the metal
- Metals are ductile and malleable
- Can be drawn out into wired due to layered structure of the lattice as they can slide over each other.
- Top layer moves and does not disrupt the bonding and can still held together the delocalised electrons
- Strong attraction between the positive ions and the delocalised electrons holds the structure together.
- Metals have high densities:
- Packed tightly together and so the density is high
- Most metals have high melting points:
- Metals have large regular structure with strong electrostatic forces
- Attraction force must be overcome in able to metal to melt so it would require a lot of heat energy.
- Strength of Metallic bonding depends on 2 factor:
- The charge on the ions
- The size of the metal ions
- The Charge on metal ions:
- The greater the charge, the greater the attraction the stronger the metallic bonds
- High charge, High melting
- The size of metal ions:
- The smaller the metal ion, the closer the nucleus is to the delocalised electrons.
- Meaning there are greater attraction between two means stronger metallic bond.