Ionic compounds do not have

Options

A. hard and brittle nature
B. high melting and boiling point
C. directional properties
D. soluble in polar solvents

Answer

### Step-by-Step Solution

**Step 1: Understanding Ionic Compounds**
Ionic compounds are formed when atoms transfer electrons from one to another, resulting in the formation of ions. These ions are held together by strong electrostatic forces of attraction, known as ionic bonds.

**Step 2: Properties of Ionic Compounds**
Ionic compounds exhibit several distinct properties:

1. **Solubility in Water**: Ionic compounds, such as sodium chloride (NaCl), are generally soluble in water. When dissolved, they dissociate into their constituent ions.

2. **Electrical Conductivity**: When ionic compounds are dissolved in water or melted, they conduct electricity. This is because the free-moving ions can carry an electric current.

3. **High Melting and Boiling Points**: Ionic compounds have high melting and boiling points due to the strong ionic bonds between the ions, which require a significant amount of energy to break.

4. **Formation of Crystals**: Ionic compounds typically form crystalline structures. The arrangement of ions in a crystal lattice maximizes the attractive forces between oppositely charged ions.

5. **Non-Directional Bonds**: Ionic bonds are considered non-directional, meaning that the force of attraction acts equally in all directions around the ion. This is different from covalent bonds, which are directional.

**Step 3: Conclusion**
In summary, ionic compounds do not exhibit certain properties that are characteristic of covalent compounds, such as low melting points, poor solubility in water, and non-conductivity in solid form. Instead, they are soluble in water, conduct electricity when dissolved or molten, have high melting and boiling points, form crystals, and have non-directional bonds.