Properties of Ionic Compounds

To learn about the properties of ionic compounds, let us perform the following Activity:

Activity 3.13

1. Take samples of sodium chloride, potassium iodide, barium chloride or any other salt from the science laboratory.
2. What is the physical state of these salts?
3. Take a small amount of a sample on a metal spatula and heat directly on the flame (Fig. 3.7). Repeat with other samples.
4. What did you observe? Did the samples impart any colour to the flame? Do these compounds melt?
5. Try to dissolve the samples in water, petrol and kerosene. Are they soluble?
6. Make a circuit as shown in Fig. 3.8 and insert the electrodes into a solution of one salt. What did you observe? Test the other salt samples too in this manner.
7. What is your inference about the nature of these compounds?

Figure 3.8

Testing the conductivity of a salt solution

You may have observed the following general properties for ionic compounds—

(i) Physical nature: Ionic compounds are solids and are somewhat hard because of the strong force of attraction between the positive and negative ions. These compounds are generally brittle and break into pieces when pressure is applied.

(ii) Melting and Boiling points: Ionic compounds have high melting and boiling points (see Table 3.4). This is because a considerable amount of energy is required to break the strong inter-ionic attraction.

(iii) Solubility: Electrovalent compounds are generally soluble in water and insoluble in solvents such as kerosene, petrol, etc.

(iv) Conduction of Electricity: The conduction of electricity through a solution involves the movement of charged particles. A solution of an ionic compound in water contains ions, which move to the opposite electrodes when electricity is passed through the solution. Ionic compounds in the solid state do not conduct

electricity because movement of ions in the solid is not possible due to their rigid structure. But ionic compounds conduct electricity in the molten state. This is possible in the molten state since the elecrostatic forces of attraction between the oppositely charged ions are overcome due to the heat. Thus, the ions move freely and conduct electricity.