• salts.
  • some salts are different from others?!

salts

  • what is a salt
  • salts are substances that form when a hydrogen acid gets replaced with a metal ion.

copper sulphate (example)

  • copper sulphate has two forms:
    • hydrated, and anhydrous
  • CuSO4 . 7H2O (s)
    • hydrated salt, water is part of the crystal.
      • the water xH2O is called water of crystallisation
      • the water has weak attractions in particular to cations.
    • not ionic bonding, heat is enough to dehydrate the compound.
      • if that occurs, white powder of CuSO4 (s) and xH2O (g) which evaporates.
      • this is called anhydrous.
    • you can calculate mass of water compounds given mass of solution and mass of anhydrous salt.
    • use since u should use moles as the unit in your calculation.

example question

  1. from the experiment results below, work out the formula of the hydrated salt.

    • mass of CaCl2 . xH2O = 6.573g

    • mass of CaCl2 = 3.333g

    • n = m/M

    • n(CaCl2) = 3.333g / (40.08 + 35.45 + 35.45)

    • => 3.333/(40.08 + 35.45 + 34.45) = 0.03003 moles (0.03003243828)

    • n(CaCl2.xH2O) = (6.573)/(16 + 16 + 1.008 + 40.08 + 35.45 + 35.45) = 0.04565 moles (0.04564963747)

    • n(xH2O) = (6.573-3.333)/(16 + 1.008 + 1.008) = 0.17984

    • 0.3003/0.3003 = 1 | 0.17984/0.03003 = 5.989 ~= 6

      mass3.3333.24
      Mr110.9818.016
      moles0.030030.17984
      ratio15.986
      CoCl2H2O
      mass0.640.532
      Mr129.8318.016
      moles0.004930.0294
      ratio16
      NiSO4H2O
      mass0.6730.471
      Mr154.7518.016
      moles0.0043489499190.02614342806
      ratio16.0114346099

covalent bonding

  • Cl2 H2O, HCl, CH3COOH, Co2, N2, O3
    • the following are all covalently bonded
    • shared electrons (called the bonding/shared pair)
    • long definition: there is electrostatic forces of attraction between the bonding pair/shared pair of electrons and nuclei of atoms at each side.
    • short definition: shared electrons between electrostatic forces of attractions.

combining power

  • the amount of hydrogen atoms required to complete the electron shell to achieve the stability of nearest noble gas.