Assertion:SiC has higher melting point than NaCl.
Reason: SiC has stronger electrostatic forces of attraction.

Options

A. If both assertion and reason are true and reason is the correct explanation of assertion
B. If both assertion and reason are true but reason is not the correct explanation of assertion.
C. If assertion is true but reason is false
D. If both assertion and reason are false

Explanation

To analyze the question, we need to evaluate both the assertion and the reason provided.

### Step-by-Step Solution:

1. **Understanding the Assertion**:
- The assertion states that SiC (Silicon Carbide) has a higher melting point than NaCl (Sodium Chloride).
- **Fact**: SiC is known to have a very high melting point, typically around 2700°C, while NaCl has a melting point of about 801°C.

2. **Understanding the Reason**:
- The reason states that SiC has stronger electrostatic forces of attraction.
- **Fact**: SiC is a covalent network solid, meaning it is held together by strong covalent bonds rather than electrostatic forces typical of ionic compounds like NaCl.

3. **Analyzing the Nature of Bonds**:
- SiC consists of covalent bonds, which are generally stronger than the ionic bonds found in NaCl.
- Ionic compounds like NaCl are held together by electrostatic forces between positively and negatively charged ions, but SiC does not primarily rely on these forces.

4. **Conclusion**:
- The assertion is true because SiC does indeed have a higher melting point than NaCl.
- The reason is false because SiC does not have stronger electrostatic forces of attraction; it has strong covalent bonds instead.

5. **Final Answer**:
- Based on the analysis, the correct option is that the assertion is true, but the reason is false.