Question

Statement 1: The correct order of 2\(^\text{nd}\) ionization energy for boron family elements is: \( \text{B}>\text{Al}>\text{Ga} \).
Statement 2: The correct order of 1\(^\text{st}\) ionization energy for carbon family elements is: \( \text{Si}>\text{Ge}<\text{Pb}<\text{Sn} \).
Choose the correct option:

• A. Both statement 1 and statement 2 are correct
• B. Statement 1 is correct and statement 2 is incorrect
• C. Statement 1 is incorrect and statement 2 is correct
• D. Both statement 1 and statement 2 are incorrect

Hint:

Ionization energy trends follow periodic patterns: it increases across a period and decreases down a group. For the boron family, the second ionization energy increases as we move from Al to Ga, but not as suggested in statement 1.

Answer 1

The Correct Option is D

Step 1: Analyzing statement 1.
The ionization energy generally increases across a period and decreases down a group. In the case of the second ionization energy for boron family elements, the order should be \( \text{B}>\text{Ga}>\text{Al} \). This is because boron has a smaller atomic size compared to aluminum and gallium, so the second ionization energy is higher for boron. The given order \( \text{B}>\text{Al}>\text{Ga} \) is incorrect.

Step 2: Analyzing statement 2.
For the first ionization energy of the carbon family elements, we know that the ionization energy decreases as we move down the group due to increasing atomic size. Therefore, the correct order should be \( \text{Si}>\text{Ge}>\text{Sn}>\text{Pb} \). The order given in statement 2, \( \text{Si}>\text{Ge}<\text{Pb}<\text{Sn} \), is incorrect.

Step 3: Conclusion.
Both statement 1 and statement 2 are incorrect. Therefore, the correct answer is option (D).
Final Answer: (D) Both statement 1 and statement 2 are incorrect