A, B, C are three substances. A does not conduct electricity in the solid, molten state and aqueous solution. B conducts electricity both in the fused and aqueous states, while C conducts electricity only in the aqueous state. In solid state neither B nor C conducts electricity. Which of the following statements is/are true regarding A, B and C ?

Options

A. A has polar covalent linkage
B. A has nonpolar covalent linkage
C. B is ionic in nature
D. Cation formed by C is highly polarizing

Answer

To analyze the properties of substances A, B, and C based on their electrical conductivity, we can break down the information provided step by step.

### Step 1: Analyze Substance A
- **Given Information**: A does not conduct electricity in solid, molten, or aqueous states.
- **Conclusion**: Since A does not conduct electricity in any state, it cannot have polar covalent bonds. The absence of conductivity implies that there are no free-moving charged particles (ions or electrons) in any of its states.

**Hint**: Remember that conductivity in substances is often linked to the presence of free-moving charged particles.

### Step 2: Analyze Substance B
- **Given Information**: B conducts electricity in both fused (molten) and aqueous states, but not in solid state.
- **Conclusion**: The ability to conduct electricity in molten and aqueous states suggests that B is ionic in nature. When B is melted or dissolved in water, it dissociates into ions, which are free to move and carry an electric current.

**Hint**: Ionic compounds typically conduct electricity when they are in a liquid state or dissolved in water due to the mobility of ions.

### Step 3: Analyze Substance C
- **Given Information**: C conducts electricity only in aqueous state and not in solid state.
- **Conclusion**: The fact that C conducts electricity only in aqueous state suggests that it may be a covalent compound that ionizes in water. This means that while C does not have free-moving ions in solid form, it can form ions when dissolved in water, allowing it to conduct electricity.

**Hint**: Some covalent compounds can ionize in water, leading to conductivity only in the aqueous state.

### Step 4: Evaluate the Statements
- **Statement 1**: A has polar covalent linkage.
- **Evaluation**: This statement is false because A does not conduct electricity in any state, indicating it does not have polar covalent bonds.

- **Statement 2**: A has non-polar covalent linkage.
- **Evaluation**: This statement is true. Since A does not conduct electricity, it likely has non-polar covalent bonds.

- **Statement 3**: B conducts electricity in fused and aqueous states, indicating it is ionic.
- **Evaluation**: This statement is true. B is ionic as it conducts electricity in these states.

- **Statement 4**: C conducts electricity only in aqueous state, indicating its cation is highly polarizing.
- **Evaluation**: This statement is likely true. The ability of C to conduct electricity only in aqueous solution suggests that it forms ions in water, and the polarizing nature of the cation supports this.

### Final Conclusion
Based on the analysis:
- **True Statements**: Statement 2, Statement 3, and Statement 4 are true.
- **False Statement**: Statement 1 is false.