bonding

• ionic bonding 


  electrost attraction between positive and negative ions
• structure of ionic compound

  giant ionic lattice
• properties of ionic compounds

  high melting and boiling points

  tend to dissolve in polar solvents such as water

  conduct electricity only in liquid state or aqueous solution
• ionic compounds melting and boiling points


  most ionic compounds are solid at rtp

  high temperatures are needed to overcome the strong electrostatic forces of attraction between ions so therefore high melting/boiling points
• ionic compounds solubility

  many ionic compounds dissolve in polar solvents such as water

  in compounds made of ions with large charges, the ionic attraction may be too strong for water to be able to break down the lattice structure so the compound wont be very soluble
• ionic compounds electrical conductivity

  does not conduct in solid state as no mobile charge carriers

  but when liquid or dissolved in water solid ionic lattice breaks down so now ions are free to move as mobile charge carriers
• covalent bonding


  strong electrostatic force of attraction between a shared pair of electrons and the nuclei of bonded atoms
• the covalent bond


  overlap of atomic orbitals each containing one electron to give a shared pair of electrons which is attracted to the nuclei of both bonding atoms
• dative covalent bonds


  covalent bond in which the shared pair of electrons has been supplied by one of the bonding atoms only(in the dative covalent bond the shared pair was originally a lone pair on one of the bonded atoms)