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Assertion(A) : IE(1) of C is greater tha...

Assertion(A) : `IE_(1)` of `C` is greater than that of `B`.
Reason (R ): Due to penetration effect the `IE_(1)` of `C` is greater than
that of `B`

A

If both Assertion (A) and (R ) are correct and Reason (R ) is the
correct explanation of Assertion (A).

B

If both (A) and (R ) are correct but (R ) is not the correct explanation
for (A).

C

If (A) is correct but (R ) is not correct.

D

If (A) is incorrect and (R ) is correct

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the assertion and reason about the first ionization energy (IE₁) of carbon (C) and boron (B), we will analyze both statements step by step. ### Step 1: Analyze the Assertion (A) The assertion states that the first ionization energy (IE₁) of carbon (C) is greater than that of boron (B). - **Explanation**: - Carbon (C) is in Group 14 of the periodic table, while boron (B) is in Group 13. - As we move from left to right across a period in the periodic table, the ionization energy generally increases. This is due to an increase in nuclear charge (the number of protons in the nucleus) which results in a stronger attraction between the nucleus and the outer electrons. - Therefore, since carbon is to the right of boron in the same period, it has a higher ionization energy. **Conclusion**: The assertion is correct. ### Step 2: Analyze the Reason (R) The reason states that the greater ionization energy of carbon compared to boron is due to the penetration effect. - **Explanation**: - The penetration effect refers to how close an electron can get to the nucleus. Electrons in s-orbitals are more penetrating than those in p-orbitals. - However, in this case, the difference in ionization energy between carbon and boron is primarily due to the increase in nuclear charge as we move from boron to carbon, rather than the penetration effect. - The outer electrons of carbon experience a stronger effective nuclear charge compared to those in boron, making it harder to remove an electron from carbon. **Conclusion**: The reason is incorrect. ### Final Conclusion - The assertion (A) is correct: IE₁ of C is greater than that of B. - The reason (R) is incorrect: The increase in ionization energy is primarily due to nuclear charge, not the penetration effect. ### Final Answer The correct answer is that the assertion is correct, but the reason is not correct. ---
To solve the question regarding the assertion and reason about the first ionization energy (IE₁) of carbon (C) and boron (B), we will analyze both statements step by step. ### Step 1: Analyze the Assertion (A) The assertion states that the first ionization energy (IE₁) of carbon (C) is greater than that of boron (B). - **Explanation**: - Carbon (C) is in Group 14 of the periodic table, while boron (B) is in Group 13. - As we move from left to right across a period in the periodic table, the ionization energy generally increases. This is due to an increase in nuclear charge (the number of protons in the nucleus) which results in a stronger attraction between the nucleus and the outer electrons. ...
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