Ionic Compounds: Properties MCQs Quiz | Class 10
This Class X Science (Code 086) quiz focuses on Unit I: Chemical Substances – Nature and Behaviour. It covers the topic of Ionic Compounds: Properties MCQs Quiz | Class 10, specifically testing knowledge on high melting points, electrical conduction, and solubility. Attempt the questions, review your score, and click the button to download your result PDF.
Overview of Ionic Compounds Properties
Ionic compounds are formed by the complete transfer of electrons from a metal to a non-metal, resulting in positive and negative ions held together by strong electrostatic forces. These forces dictate their physical and chemical properties.
Key Properties
- Physical Nature: Ionic compounds are typically solid and hard due to the strong force of attraction between the positive and negative ions. However, they are generally brittle and break into pieces when pressure is applied.
- Melting and Boiling Points: They have high melting and boiling points because a considerable amount of energy is required to break the strong inter-ionic attraction.
- Solubility: Electrovalent compounds are generally soluble in water (polar solvents) and insoluble in solvents such as kerosene and petrol (non-polar solvents).
- Conduction of Electricity: Conduction of electricity 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. In the solid state, ionic compounds do not conduct electricity because movement of ions is not possible due to their rigid structure. However, they conduct electricity in the molten state.
Comparison Table
| Property | Ionic Compounds |
|---|---|
| State | Solid, Hard, Brittle |
| Melting Point | High |
| Electrical Conduction | Good in molten/aqueous state; Poor in solid |
| Solubility | High in water; Low in organic solvents |
Quick Revision Points
- The force binding ions is the electrostatic force of attraction.
- Ions must be free to move for electricity to flow.
- Water weakens the electrostatic forces, allowing ions to separate and conduct electricity.
- Lattice energy is high, requiring high heat to melt the compound.
Extra Practice Questions
- Why does Sodium Chloride have a high melting point?
- Explain why ionic compounds conduct electricity in water but not as solids.
- What happens when pressure is applied to an ionic crystal?
- Why is Calcium Oxide soluble in water but not in petrol?
- Define the term ‘Electrostatic Force’ in the context of ionic bonds.
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