Module 2- Types of Bonding

Cards (10)

  • Ionic
    The electrostatic attraction between positive and negative ions
  • Ionic compounds are solid at room temperature with high melting and boiling points because a large amount of energy is needed to break the strong electrostatic forces of attraction holding the opposite ions together.
  • Ionic compounds cannot conduct electricity when solid because the ions are in a fixed position.
  • Ionic compounds when dissolved in water or molten are good conductors as ions are free to move so electricity can flow.
  • Ionic compounds are soluble in polar solvents.
  • Covalent Bonding

    Strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms.
  • Giant Covalent Lattices
    Many atoms bonded together by covalent bonds. (Diamond/Graphite/Graphene)
  • Diamond
    • 4 carbons
    • tetrahedral shape
    • strong covalent bonds
    • high melting point
    • poor conductor
    • insoluble in water
  • Graphite
    • 3 carbons
    • trigonal planar shape
    • layered with delocalised electrons between
    • high melting point
    • strong covalent bonds
    • good conductor
    • insoluble in water
    • weak forces holding layers
  • Graphene
    • 3 carbons
    • sheet of carbons in hexagons
    • one atom thick
    • best conductor of electricity
    • high melting and boiling point
    • transparent and incredibly light