Which of the following lists includes all the types of intermolecular forces that can affect the properties of H2S?

• A. Only London dispersion forces
• B. London dispersion forces and dipole-dipole interactions
• C. Hydrogen bonding and London dispersion forces
• D. Dipole-dipole interactions and hydrogen bonding

Answer: (B)

Verified step by step guidance

1. Step 1: Identify the molecular structure and polarity of H\_2S. H\_2S is a bent molecule with sulfur bonded to two hydrogen atoms. Since sulfur is more electronegative than hydrogen, the molecule has polar bonds, resulting in a net dipole moment, making H\_2S a polar molecule.
2. Step 2: Determine the types of intermolecular forces possible for H\_2S. Because it is a polar molecule, it can exhibit dipole-dipole interactions. Additionally, all molecules experience London dispersion forces due to temporary fluctuations in electron density.
3. Step 3: Consider whether hydrogen bonding is possible. Hydrogen bonding occurs when hydrogen is directly bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine. Since sulfur is less electronegative and not one of these atoms, H\_2S does not exhibit hydrogen bonding.
4. Step 4: Summarize the intermolecular forces affecting H\_2S. The molecule experiences both London dispersion forces (present in all molecules) and dipole-dipole interactions (due to its polarity), but not hydrogen bonding.
5. Step 5: Conclude that the correct list of intermolecular forces for H\_2S includes London dispersion forces and dipole-dipole interactions only.