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Assertion:- Boiling point of cis-2-buten...

Assertion:- Boiling point of cis-2-butene is more than trans-2-butene.
Reason:- Dipole moment of cis-2-butene is more than
trans-2-butene.

A

If both Assertion `&` Reason are True `&` the Reason is a correct explanation of the Assertion.

B

If both Assertion `&` Reason are True but Reason is not a correct explanation of the Assertion.

C

If Assertion is True but the Reason is False.

D

If both Assertion `&` Reason are False.

Text Solution

AI Generated Solution

The correct Answer is:
To solve the assertion and reason question regarding the boiling points of cis-2-butene and trans-2-butene, we will analyze both statements step by step. ### Step 1: Understand the Assertion **Assertion:** Boiling point of cis-2-butene is more than trans-2-butene. - **Explanation:** The boiling point of a substance is influenced by its molecular structure and the interactions between its molecules. In this case, we need to compare the boiling points of cis-2-butene and trans-2-butene. ### Step 2: Understand the Reason **Reason:** Dipole moment of cis-2-butene is more than trans-2-butene. - **Explanation:** The dipole moment is a measure of the polarity of a molecule. Polarity arises from the distribution of electrical charge across the molecule. In cis-2-butene, the two methyl (CH₃) groups are on the same side of the double bond, creating a net dipole moment. In contrast, in trans-2-butene, the methyl groups are on opposite sides, which cancels out the dipole moments, resulting in a net dipole moment of zero. ### Step 3: Compare the Dipole Moments - **Cis-2-butene:** Has a net dipole moment due to the arrangement of groups leading to a polar molecule. - **Trans-2-butene:** Has no net dipole moment as the dipole moments cancel each other out, making it non-polar. ### Step 4: Relate Dipole Moment to Boiling Point - Polar molecules tend to have stronger intermolecular forces (like dipole-dipole interactions), which leads to higher boiling points. Since cis-2-butene is more polar than trans-2-butene, it will have stronger dipole-dipole interactions. ### Step 5: Conclusion - Therefore, the boiling point of cis-2-butene is indeed higher than that of trans-2-butene due to its higher dipole moment, which leads to stronger intermolecular forces. ### Final Answer Both the assertion and reason are true, and the reason correctly explains the assertion. ---
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Knowledge Check

  • Cis-2-butene and trans-2-butene are.

    A
    geometrical isomers
    B
    diastereomers
    C
    enantiomers
    D
    position isomers

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