Question

Given below are two statements :

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

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

Hint:

Pay close attention to the exact structures and comparisons made in the statements. Even if the underlying chemical principles are correct, a flawed comparison in the statement makes the statement incorrect.

Answer 1

The Correct Option is A

To determine the correctness of the statements, let's analyze each one:

1. Statement I: The structure with chlorine (Cl) atoms is more polar than the structure with bromine (Br) atoms.
   • Chlorine is more electronegative than bromine. Electronegativity influences polarity, as higher electronegativity leads to higher polarity when atoms are involved in bonds.
   • Given this, the molecule with chlorine will be more polar than the one with bromine.
   • Hence, Statement I is correct.
2. Statement II: The boiling point of the bromine-containing structure is lower than the structure with di-bromo substitution, but the first is more polar.
   • Boiling points depend significantly on molecular weight and intermolecular forces. Bromine atoms make a compound heavier and usually increase van der Waals forces.
   • Thus, the boiling point of a fully substituted bromo compound is generally higher than that of a compound with fewer bromine atoms.
   • Additionally, more polarity in bromine-containing compounds doesn't necessarily correlate with lower boiling points if molecular weight is increased.
   • Hence, Statement II is incorrect.

Based on the analysis above, the most appropriate answer is: Statement I is correct but Statement II is incorrect.

Answer 2

Step 1: Analyze Statement (I).
As established previously, the C-Cl bond is more polar than the C-Br bond due to the higher electronegativity of chlorine. In the \( \textit{cis } \) isomers, the bond dipoles have a net vector sum, resulting in a polar molecule. Since the C-Cl bond is more polar, \( \textit{cis}-1,2-dichloroethene \) will have a larger net dipole moment and thus be more polar than \( \textit{cis}-1,2-dibromoethene \). Statement I is correct.
Step 2: Analyze Statement (II).
The first part of Statement II is correct: \( \textit{trans}-1,2-dibromoethene \) is nonpolar (due to the cancellation of bond dipoles), and \( \textit{cis}-1,2-dibromoethene \) is polar. Polar molecules generally have stronger intermolecular forces (dipole-dipole interactions) compared to nonpolar molecules (van der Waals forces of similar magnitude), leading to higher boiling points. Thus, the boiling point of \( \textit{trans}-1,2-dibromoethene \) is lower than that of \( \textit{cis}-1,2-dibromoethene \). The second part of Statement II claims that \( \textit{cis}-1,2-dibromoethene \) is more polar than \( \textit{trans}-1,2-dibromoethene \). \( \textit{cis}-1,2-dibromoethene \) has a net dipole moment (it is polar), while \( \textit{trans}-1,2-dibromoethene \) has a zero net dipole moment (it is nonpolar). Therefore, \( \textit{cis}-1,2-dibromoethene \) is more polar than \( \textit{trans}-1,2-dibromoethene \). However, the structure provided in Statement II has a typo. It shows \( \textit{trans}-1,2-dibromoethene \) being compared to another molecule that is also \( \textit{trans}-1,2-dibromoethene \), making the comparison meaningless. Assuming the second molecule in the polarity comparison was intended to be \( \textit{cis}-1,2-dibromoethene \), then the statement "it is more polar than \( \textit{trans}-1,2-dibromoethene \)" would be correct. Given the figure as presented, Statement II makes an incorrect comparison for polarity. Therefore, Statement II is incorrect as written.
Step 3: Determine the correctness of both statements.
Statement I is correct, but Statement II is incorrect as presented in the figure.
Step 4: Choose the appropriate option.
The option that states Statement I is correct but Statement II is incorrect is (1).