structure types

• Monatomic Structures 


  group 0
• monatomic structures

  structure: individual atoms with very weak forces between them
• monatomic structures


  do not conduct electricity, no charged particles that can move, atoms are neutral
• monatomic structures


  solubility: insoluble
• covalent bonds

  non-metals
• ionic

  non-metals and metals
• metallic

  metals
• simple molecular 


  structure:

  lots of individual molecules with weak forces between the molecules. atoms within molecules are bonded by covalent bonds.

  solid: lattice structure held together by weak intermolecular forces
• simple molecular 


  low boiling/melting point due to weak intermolecular forces
• simple molecular


  do not conduct electricity as the molecules are neutral
• simple molecular structures are usually insoluble
• giant covalent structures have a lattice structure in which all atoms are joined together in a giant network by covalent bonds
• giant covalent structures have very high melting and boiling points because of the strong covalent bonds
• giant covalent structures do not conduct electricity because there are no delocalized electrons, except from graphene and graphite where delocalized electrons move between layers of atoms
• giant covalent structures are insoluble
• ionic structures are made from metals and non-metals
• ionic structures


  lattice structures of positive and negative ions held together by ionic bonding
• ionic structures have high boiling and melting points because of the strong electrostatic attraction between positive and negative ions.
• ionic structures only conduct electricity when molten or dissolved in water but do not conduct electricity when solid
• ionic compounds are usually soluble
• metallic structures


  metallic structures lattice structure of metal atoms where the outer shell electrons from each atom are delocalized so they can conduct electricity
• metallic structures have high melting/ boiling points due to the strong metallic bonds
• metallic structures are insoluble
• atoms form bonds to get a full outer shell in order to become stable
• group 1 


  1+ ions
• group 2 


  2+ ions
• group 6 


  2- ions
• group 7


  form -1 ions
• graphene 


  single layer of graphite
• fullerenes 


  molecules of carbon atoms with hollow shapes
• carbon nanotube 


  a cylindrical fullerene with a very high length to diameter ratio
• ionic bonding


  metal atom loses electrons to form a positively charged ion and the non metal gains these electrons to form a negatively charged ion, the oppositely charged ions are strongly attracted to one another by electrostatic forces of attraction
• covalent bonding 


  non-metal atoms share electrons to make covalent bonds that are very strong
• metallic bonding 


  the electrons in the outer shell of metal atoms are delocalized. there are strong forces of electrostatic attraction between the positive metal ions and the shared negative electrons. these forces of attraction hold the atoms together in a regular structure. metallic bonds are very strong.