Bonding summary

• Diatomic elements


  • Hydrogen
  • Nitrogen
  • Oxygen
  • Fluorine
  • Chlorine
  • Bromine
  • Iodine
• Diatomic elements


  Exist as diatomic molecules through the formation of covalent bonds
• Bonding


  The attractive forces between atoms, ions or molecules in a compound
• Diagram


  A visual representation of bonding and structure
• Melting Point (M.Pt)


  The temperature at which a solid becomes a liquid
• Boiling Point (B.Pt)


  The temperature at which a liquid becomes a gas
• State at Room Temp

  The physical state of a substance at room temperature (25 degrees Celsius)
• Soluble in Water?


  • Yes
  • No
• Conducts Electricity?


  • Yes
  • No
• Monoatomic elements


  • Noble gases
• Noble gases


  • He, Ne
• Covalent molecular bonding


  Atoms share electrons to form a molecule
• Examples of covalent molecular bonding

  • N
  • CO
  • H2O
• Weak intermolecular forces


  Attractive forces between molecules that are weaker than covalent or ionic bonds
• Examples of weak intermolecular forces

  • Small molecules
  • Low boiling point gases
• Van der Waals forces

  A type of weak intermolecular force
• Examples of solid Van der Waals forces

  • G, B, Si
• Diamond structure


  A covalent network structure with strong bonds in three dimensions
• Examples of diamond structure


  • Graphite
• Examples of ionic lattice bonding


  • Na Cl
  • An Ha
• Metallic lattice bonding


  Metal atoms lose electrons to form a lattice with delocalised electrons
• Examples of metallic lattice bonding


  • ZA
• Conducts electricity as


  • Solid
  • Liquid
  • Gas
• Conducts electricity as solid

  • Yes (except graphite)
• Conducts electricity as liquid or solid

  • Yes