Which types of intermolecular forces are present in dichloromethane (CH2Cl2)?

• A. London dispersion forces only
• B. London dispersion forces and dipole-dipole interactions
• C. Hydrogen bonding only
• D. Hydrogen bonding and dipole-dipole interactions

Answer: (B)

Verified step by step guidance

1. Identify the molecular structure of dichloromethane (CH2Cl2). It consists of a central carbon atom bonded to two hydrogen atoms and two chlorine atoms.
2. Determine the polarity of the molecule by considering the electronegativity differences between carbon, hydrogen, and chlorine atoms. Chlorine is more electronegative than carbon and hydrogen, creating polar C-Cl bonds.
3. Recognize that because the molecule has polar bonds arranged asymmetrically, it has a net dipole moment, meaning dipole-dipole interactions are present.
4. Recall that all molecules, regardless of polarity, exhibit London dispersion forces due to temporary fluctuations in electron density.
5. Evaluate the possibility of hydrogen bonding: hydrogen bonding requires hydrogen directly bonded to highly electronegative atoms like N, O, or F. Since CH2Cl2 has no such bonds, hydrogen bonding is not present.