Question:
Given below are two statements:
Statement I: The second ionization enthalpy of B, Al and Ga is in the order of B>Al>Ga.
Statement II: The correct order in terms of first ionization enthalpy is Si<Ge<Pb<Sn.
In light of the above statements, choose the correct answer from the options given below:
Given below are two statements:
Statement I: The second ionization enthalpy of B, Al and Ga is in the order of B>Al>Ga.
Statement II: The correct order in terms of first ionization enthalpy is Si<Ge<Pb<Sn.
In light of the above statements, choose the correct answer from the options given below:
Statement II: The correct order in terms of first ionization enthalpy is Si<Ge<Pb<Sn.
In light of the above statements, choose the correct answer from the options given below:
Updated On: Apr 10, 2026
- Both Statement I and Statement II are true.
- Both Statement I and Statement II are false.
- Statement I is true but Statement II is false.
- Statement I is false but Statement II is true.
Show Solution
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The Correct Option is C
Solution and Explanation
Statement I is correct. The second ionization enthalpy of elements generally increases across a period, and for B, Al, and Ga, the second ionization enthalpy follows the order B>Al>Ga.
Statement II is false. The correct order in terms of first ionization enthalpy is Si<Ge<Sn<Pb, not as mentioned in the question. Thus, Statement II is incorrect.
Final Answer: (C) Statement I is true but Statement II is false.
Statement II is false. The correct order in terms of first ionization enthalpy is Si<Ge<Sn<Pb, not as mentioned in the question. Thus, Statement II is incorrect.
Final Answer: (C) Statement I is true but Statement II is false.
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