Assertion (A) : Carbon forms covalent compounds but lead dorms ionic compounds
Reason (R) : carbon can lose four electrons to four `C^(4+)` ion but lead cannot .

Options

A. If both (A) and (R) are correct and (R) is correct explanation of (A)
B. If both (A) and (R) are correct and (R) is not correct explanation of (A)
C. If (A) is correct , but (R) is incorrect
D. If (A) is incorrect but (R) is correct

Explanation

### Step-by-Step Solution:

1. **Understanding the Assertion (A)**:
- The assertion states that "Carbon forms covalent compounds but lead forms ionic compounds."
- Carbon, being a non-metal, typically forms covalent bonds by sharing electrons. Lead, being a heavier element and more metallic in character, tends to lose electrons and form ionic bonds.

2. **Analyzing the Reason (R)**:
- The reason states that "Carbon can lose four electrons to form C^(4+) ion but lead cannot."
- This statement is incorrect. While carbon can indeed form covalent bonds by sharing its four valence electrons, it does not typically form a C^(4+) ion. Instead, it can form a C^(4-) ion when it gains electrons, but this is not common. Lead, on the other hand, can lose electrons to form cations (like Pb^(2+) or Pb^(4+)), which is consistent with its metallic character.

3. **Conclusion**:
- The assertion is true because carbon does form covalent compounds while lead forms ionic compounds.
- The reason is false because it misrepresents the behavior of carbon and lead regarding electron loss and ion formation.
- Therefore, the correct answer is that the assertion is true, but the reason is false.

### Final Answer:
- Assertion (A) is true, and Reason (R) is false.