Question

Given below are two statements:


Statement (II): Structure III is most stable, as the orbitals having the lone pairs are axial, where the $ \ell p - \beta p $ repulsion is minimum. In light of the above statements, choose the most appropriate answer from the options given below:

• A. Statement I is incorrect but Statement II is correct
• B. Statement I is correct but Statement II is incorrect
• C. Both Statement I and Statement II are correct
• D. Both Statement I and Statement II are incorrect

Hint:

In reactions involving lone pairs, remember that in \( sp^3d \) hybridization, lone pairs prefer equatorial positions to minimize \( \ell p - \beta p \) repulsion, not axial positions.

Answer 1

The Correct Option is B

To solve this question, we need to evaluate the given statements regarding the stability of the structures of \(ClF_3\). The question includes three structures labeled I, II, and III, and we must determine the validity of Statements I and II.

1. Statement I: This statement claims that for \(ClF_3\), all three possible structures can be drawn. This is indeed correct. \(ClF_3\) has a trigonal bipyramidal molecular geometry with two lone pairs of electrons. The lone pairs will occupy the equatorial positions to minimize repulsion, resulting in these three possible structures.
2. Statement II: This statement argues that Structure III is the most stable because the orbitals with lone pairs are axial, minimizing \(\ell p - \beta p\) (lone pair - bond pair) repulsion. However, this is incorrect because in a trigonal bipyramidal arrangement, the lone pairs prefer to occupy the equatorial positions due to lesser repulsion with bond pairs. This means that Structure I, where lone pairs are equatorial, is more stable than Structure III.

Conclusion: From the above analysis, it is clear that Statement I is correct, whereas Statement II is incorrect. Therefore, the most appropriate answer is: Statement I is correct but Statement II is incorrect.

Answer 2

Analysis of the Given Statements:

Statement I: For \(\text{ClF}_3\), all three possible structures are shown in the diagram. This statement is correct. Chlorine trifluoride (\(\text{ClF}_3\)) is known to exist in three different structures based on the arrangement of the lone pairs and bonding pairs.

Statement II: Claims that structure III is the most stable due to the lone pairs being axial, reducing \(\ell p - \beta p\) (lone pair-bond pair) repulsion.

Explanation:

1. In \(\text{ClF}_3\), chlorine has five electron pairs (3 bonding with fluorine and 2 lone pairs), typically giving a T-shaped molecular geometry.
2. The stability of these structures is influenced primarily by the arrangement of lone pairs to minimize repulsion.
3. Structure II is known to be the most stable configuration due to its T-shape where lone pair-bond pair repulsions are minimized compared with structure III.

Conclusion: Statement I is correct as it accurately describes the possible structures. However, Statement II is incorrect; structure III is not the most stable due to its lone pair-lone pair repulsions being more significant than in structure II.

Correct Answer: Statement I is correct but Statement II is incorrect.