Ionic, Covalent, and Metallic Bonds

• Metals are malleable which means they can be moulded and shaped
• Physical properties of metals

  • Can conduct electricity
  • Metallic
  • High melting and boiling points
  • Solid at room temperature
  • Hard
  • Sonorous
  • Ductile & malleable
• Uses for Diamonds

  • Saws
  • Drills
  • Jewellery
• A mixture of foreign metals makes metals more resistant to corrosion, stronger, harder, and shinier.
• Ionic compounds conduct electricity in liquid (molten) state as ions are free moving
• Covalent compounds have low melting and boiling points due to weak intermolecular forces
• Metal atoms have valence electrons that can move within the metal lattice structure
• Properties of Ionic Compounds

  • Crystalline
  • High melting and boiling points
  • Solids at room temperature
  • Conduct electricity in liquid (molten) state
• Metals have high melting points due to strong electrostatic forces in the metal lattice structure
• Foreign atoms in a metal lattice structure can make the metal stronger and harder
• Properties of Covalent Compounds

  • Low melting and boiling points
  • Volatile (turns into gas)
  • Poor electrical conductivity
  • Weak molecular forces
• Covalent compounds cannot conduct electricity
• Metal layers can slide over each other when pulled, making the metal 'soft'
• Metal atoms can conduct a current due to the movement of valence electrons
• Metal lattice structure has delocalised electrons that make metals good conductors of electricity
• Covalent bonds are formed between non-metal atoms by sharing a pair of electrons
• Ionic compounds have a giant lattice structure