KCET · Chemistry · General Organic Chemistry
\(\text{C}-\text{Cl}\) bond in methyl chloride compared to \(\text{C}-\text{Cl}\) bond in chlorobenzene is
- A Longer and stronger
- B Shorter and stronger
- C Shorter and weaker
- D Longer and weaker
Answer & Solution
Correct Answer
(D) Longer and weaker
Step-by-step Solution
Detailed explanation
In chlorobenzene, the lone pair of electrons on the chlorine atom is in conjugation with the \(\pi\)-electron system of the benzene ring. This resonance imparts a partial double bond character to the \(\text{C}-\text{Cl}\) bond.
In methyl chloride, no such resonance is possible, and the \(\text{C}-\text{Cl}\) bond is a pure single bond.
Due to the partial double bond character, the \(\text{C}-\text{Cl}\) bond in chlorobenzene is shorter and stronger than a pure single bond.
Therefore, the \(\text{C}-\text{Cl}\) bond in methyl chloride is longer and weaker compared to the \(\text{C}-\text{Cl}\) bond in chlorobenzene.
Answer: Longer and weaker
In methyl chloride, no such resonance is possible, and the \(\text{C}-\text{Cl}\) bond is a pure single bond.
Due to the partial double bond character, the \(\text{C}-\text{Cl}\) bond in chlorobenzene is shorter and stronger than a pure single bond.
Therefore, the \(\text{C}-\text{Cl}\) bond in methyl chloride is longer and weaker compared to the \(\text{C}-\text{Cl}\) bond in chlorobenzene.
Answer: Longer and weaker
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