bonds

• Ionic bonds


  Transfer of electrons
• Opposite Charges


  • Atoms lose or gain electrons
  • Attracted to each other by electrostatic forces
• Ionic bond


  Reaction where atoms need to make full outer shell
• Metal transfers electrons to non-metals

  To form ionic bonds
• Ionic bonds require one or more equations to form
• Ionic compounds


  Each ion is attracted to all those around it
• Ionic compounds


  • Have a regular lattice structure
• Properties of ionic compounds

  • High melting and boiling points
  • Determined by the strength of the bonds holding the substance together
  • Require a lot of energy to break the many ionic bonds (high temps)
  • Conduct electricity when melted or dissociated (any charged particles that can move)
  • Cannot conduct electricity when solid (ions fixed in lattice structure)
• Ionic compounds have a regular lattice structure
• Ionic compounds have high melting and boiling points
• The properties of ionic compounds are determined by the strength of the bonds holding the substance together
• It requires a lot of energy to break the many ionic bonds in ionic compounds, which is why they have high melting and boiling points
• Ionic compounds conduct electricity when melted or dissociated, as there are charged particles that can move
• Ionic compounds cannot conduct electricity when solid, as the ions are fixed in a lattice structure and cannot move
• Accotrope


  Different structural forms of the same element in the same physical state
• Diamond


  • Strong
  • High melting point
• Diamond structure


  Each carbon atom is covalently bonded to 4 other carbon atoms
• Diamond does not conduct electricity, no electrons/ions
• Graphite


  • Soft
  • Layers held together weakly, no covalent bonds
  • Easy to slide over each other
  • High melting point
  • Delocalised electrons can conduct electricity
• Metallic bonding


  • Metacs-mutars
  • Disrupts the regular
  • Structure
• Metallic structure


  • Allos - 2 or more different elements
  • Much harder than made from individual elements
  • Giant structure of atoms arranged in a regular pattern
  • Atoms share electrons with other atoms in the metallic structure
• Metallic bonding results in high melting and boiling points, strength, and conductivity
• Metallic bonding is caused by the electrostatic attraction between the positive metal ions and the delocalized electrons
• Metallic bonding holds the atoms together in a rigid, regular pattern
• Metals are good conductors of electricity
• Metals are malleable and can be bent or hammered into shape