Describe any patterns observed in ΔH for the chloride salts. Is there a periodic trend in DH for the Group I chloride salts? Describe the trend. Ionic SolidLithium chlorideCalcium chloridePotassium chlorideSodium chlorideCalculation((401.664J/0.500g)*42.391)/1000((364.008J/0.500g)*110.98)/1000((-112.968J/0.500g)*74.55)/1000((-33.472J/0.500g)*58.44)/1000AH Rxn (kJ/mol)3481-17-3.9

To describe a relation ship in the enthalpy of dissolution of the chloride salts given the following data. The enthalpy of the dissolution for the group I chlorides is given as follows: Group I chloride ∆H LiCl 34 kJ/mol NaCl -3.9 kj/mol KCl -17 kJ/mol From the above it could be said that the enthalpy of dissolution of group I chloride will decrease on going down the group. This is due to the fact that the on going down the group, the size of the group I metal will increase which will results in a decrease in the ionization enthalpy of the group I metals. The decrease in ionization enthalpy will facilitate the removal of the outermost electron from the metal and increase its solubility. Hence since on going down the group, the solubility of the salt is increasing and the enthalpy of dissolution is decreasing. Now on comparing the enthalpy of dissolution of potassium chloride and calcium chloride, it can be observed that the enthalpy of dissolution is increasing on going from left to right in a period. Metal chloride ∆H KCl -17 CaCl2 81 This increase in enthalpy of dissolution is due to an increase in the charge present on the cation on going from left to right along a period. The increase in charge will results in an increase in the electrostatic interaction between the cation and the anion and hence will results in an increase in the energy required to separate the cations and anion that is enthalpy of dissolution.