Question

Given below are two statements: 
Statement (I): The first ionization energy of Pb is greater than that of Sn. 
Statement (II): The first ionization energy of Ge is greater than that of Si. 

In light of the above statements, choose the correct answer from the options given below:

• A. Statement I is true but Statement II is false
• B. Both Statement I and Statement II are false
• C. Statement I is false but Statement II is true
• D. Both Statement I and Statement II are true

Hint:

Ionisation energy generally decreases down a group due to increasing atomic size and distance of electrons from the nucleus.

Answer 1

The Correct Option is C

- Statement (I) is false: The ionization energy of Pb is less than that of Sn due to Pb's lower position and larger atomic size in the periodic table.
- Statement (II) is true: Ge exhibits a higher ionization energy than Si because it is positioned above Si in the same group, resulting in its electrons being closer to the nucleus.

Final Answer: Statement I is false; Statement II is true.