1. To begin with iodine monochloride is considered a covalent bond and potassium iodide is considered an ionic bond. Iodine monochloride is a bond in which valence electrons are shared and is influenced by the electrostatic force between one valence electron on one atom and a neighbouring nucleus. Potassium iodide is a bond between a cation and anion and involved the exchanging of electrons. The bond is held together due to the electrostatic force between the constituent particles. 2. Ionic compounds usually have high melting and boiling points because of the electrostatic interaction between oppositely charged ions. It takes a large amount of hear energy to overcome the attractions between ions, hence the high melting points. To convert a liquid to a gas, it is necessary to overcome all of the electrostatic interactions between oppositely charge ions. 3. The less electronegative an ionic compound is, the lower boiling and melting point an ionic compound will present. It is also observed that the more distance between the two elements ionically bonded will result in a lower boiling and melting point 4. a. Caesium and Iodine = Ca^1++ I^1- b. Aluminium and Flourine = Al^3++ F^1- c. Gallium and Oxygen = Ga^3++ O^2- d. Lithium and Nitrogen = Li^1+ + N^3- e. Sulphur and Sodium = Na^1+ + S^3- f. Bromine and Calcium = Ca^2- + B^3- 5. Sodium and Chlorine, once ionically bonded, form a strong, tight bond together, a unique pattern repeating in all directions, creating a three-dimensional, crystalline lattice structure. Because of this strong electrostatic force in Sodium Chloride, which is lacking in, Caesium Iodide, for example (because it has more electron shells), this means that the ionic compound has a high melting point and boiling point. However, compared to silver, for example (a metallic bond), that successfully conducts electricity, Sodium Chloride does not conduct electricity because the ions are held in a rigid lattice and cannot move freely to carry electrical charge. However, Sodium Chloride can conduct electricity as a molten liquid. This is because the ions are no longer in a rigid lattice but are instead freer to move between the electrodes.