Question:

Write any three general properties of ionic compounds.

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Ionic compounds have strong electrostatic forces, leading to high melting points. They conduct electricity only in molten or dissolved state due to free-moving ions.
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Solution and Explanation

Step 1: Understanding ionic compounds
- Ionic compounds are formed due to the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions). - This strong attraction gives ionic compounds unique properties.
Step 2: General properties of ionic compounds
1. High melting and boiling points: - Ionic bonds are strong and require a large amount of energy to break. - This results in high melting and boiling points. - Example: Sodium chloride (\(\text{NaCl}\)) has a high melting point of \(801^\circ C\). 2. Solubility in water: - Ionic compounds dissolve in polar solvents like water. - Water molecules separate the positive and negative ions, allowing them to disperse. 3. Electrical conductivity in molten or dissolved state: - In solid form, ionic compounds do not conduct electricity because ions are fixed in a lattice. - In molten or aqueous solution, the ions are free to move, allowing them to conduct electricity. Thus, ionic compounds exhibit high melting points, solubility in water, and electrical conductivity in liquid state.
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