Question
State the general properties of ionic compounds.
✓
Answer
The general (common) properties of ionic compounds are as follows:
(1) Physical nature: The ionic compounds are solids and hard because of the strong forces of attraction between the positive and negative ions. These compounds are generally brittle and break into pieces when pressure is applied.
(2) Melting and boiling points: A considerable large amount of energy is required to break the strong inter-ionic attraction. Hence, ionic compounds have high melting and boiling points.
For example,
Melting and boiling points of some ionic compounds
(3) Solubility: Electrovalent (Ionic) compounds are generally soluble in polar solvent like water and insoluble in non-polar organic solvents such as kerosene, petrol, etc.
(4) 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 the movement of ions in the solid is not possible due to their rigid structure. But, ionic compounds conduct electricity in the molten state. Since the electrostatic forces of attraction between the oppositely charged ions are overcome and free ions are obtained due to heat. As a result, these ions move freely and conduct electricity.
(1) Physical nature: The ionic compounds are solids and hard because of the strong forces of attraction between the positive and negative ions. These compounds are generally brittle and break into pieces when pressure is applied.
(2) Melting and boiling points: A considerable large amount of energy is required to break the strong inter-ionic attraction. Hence, ionic compounds have high melting and boiling points.
For example,
Melting and boiling points of some ionic compounds
| Ionic compound | Melting point (K) | Boiling point (K) |
| NaCl | 1074 | 1686 |
| LiCl | 887 | 1600 |
| $CaCl _2$ | 1045 | 1900 |
| CaO | 2850 | 3120 |
| $MgCl _2$ | 981 | 1685 |
(3) Solubility: Electrovalent (Ionic) compounds are generally soluble in polar solvent like water and insoluble in non-polar organic solvents such as kerosene, petrol, etc.
(4) 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 the movement of ions in the solid is not possible due to their rigid structure. But, ionic compounds conduct electricity in the molten state. Since the electrostatic forces of attraction between the oppositely charged ions are overcome and free ions are obtained due to heat. As a result, these ions move freely and conduct electricity.
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