Bonding, structure and properties

• Ion


  An atom with a positive or negative charge; they lost or gained an electron
• Metal ions


  Loose electrons so positively charged
• Non-metal ions


  Gain electrons so negatively charged
• Ionic bonding forms ions and ionic lattices
• Ionic bonding


  metal and non-metal
• Ionic bonding


  Dot and cross diagram

  (remember to put brackets and charge)
• Ionic lattice


  Regular pattern with oppositely charged ions next to eachother- strong electrostatic forces
• ionic compounds 


  High melting point

  High boiling point

  solid at room temp
• Ionic compounds can conduct electricity when

  Melted

  or dissolved in a solution
• Solid


  Particles very close

  regular pattern

  particles vibrate in a fixed position

  Low energy
• Liquid


  Particles close together

  randomly arranged

  move around each other

  greater energy
• Gas


  particles far apart

  randomly arranged

  move quickly in all directions

  highest energy
• Solids


  Cannot flow

  cannot be compressed
• Liquids


  Flow and take the shape of the container

  cannot be compressed
• Gases


  Flow and completely fill the container

  can be compressed
• Solid to liquid


  Melting
• Liquid to gas

  Evaporation
• Liquid to solid


  Freezing
• Gas to liquid 


  Condensation
• Solid to gas


  Sublimation
• Covalent bonds


  Non-metal and non-metal
• covalent bonds


  Two atoms share a pair of electrons
• Molecule


  Group of two or more atoms joined together by covalent bonds
• Giant covalent molecules 


  High melting and boiling point

  cannot conduct electricity (except graphite)
• Diamond


  Giant covalent structure

  each atom joined by 4 bonds

  regular tetrahedral structure

  no free electrons
• Graphite

  Giant covalent structure

  each arom joined by 3 bonds

  layers of hexagonal rings

  no covalent bonds between layers

  mine delocalised electron from each atom
• Graphite 


  Can conduct electricity

  weak intermolecular forces between layers so slippery - used as lubricant or in pencils
• Graphene


  Single layer of graphite

  high melting point

  very strong
• Fullerenes


  Molecules of carbon atoms with hollow shapes
• Fullerene Examples


  Buckminsterfullerene (Bucky balls)

  Nanotubes
• Buckminsterfullerene


  (Bucky balls)

  60 carbon atoms joined

  spherical

  Weak intermolecular forces

  low melting point
• Nanotubes


  Layer of Graphene rolled into a tube

  Very long

  High tension, resist being stretched

  Conduct electricity
• Polymer


  Large molecules in long chains
• Polymers


  Solid at room temp

  Strong intermolecular forces
• Metalic bonding 


  Metal and metal

  ”sea“ of delocalised electrons
• Metals


  Conduct electricity and heat

  High melting and boiling points
• Alloys


  Mixture of a metal and other elements
• Alloys


  Harder than pure metals as different size atoms disturb the regular pattern and make the layers not be able to slide over eachother