Methylene chloride (CH2Cl2) has fewer chlorine atoms than chloroform (CHCl3). Nevertheless, methylene chloride has a larger mole

Answer:

See below for the explanation.

Explanation:

• Chloroform features three C-Cl bonds that are polar, while methylene chloride contains just two of these polar bonds. Therefore, chloroform is anticipated to be more polar and have a greater dipole moment when compared to methylene chloride.
• Two factors account for the unexpected trend in dipole moments between methylene chloride and chloroform.
• The first factor is the quantity of hyperconjugative hydrogen atoms in each molecule. Hyperconjugation is associated with the empty d-orbital in the chlorine atom. This process enhances the charge separation within a molecule, leading to a higher dipole moment.
• Methylene chloride has two hyperconjugative hydrogens, while chloroform has just one. Thus, methylene chloride is expected to exhibit greater charge separation than chloroform.
• The second factor is the induction of opposing polarity in a C-Cl bond due to another C-Cl bond present within the same molecule. The greater the opposing polarity induction, the less the charge separation, resulting in a lower dipole moment overall.
• Since chloroform has three C-Cl bonds compared to the two in methylene chloride, it experiences greater opposing polarity induction, which leads to its reduced dipole moment.