Which types of intermolecular forces are present in SF_4 (sulfur tetrafluoride)?

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

Answer: (C)

Verified step by step guidance

1. Identify the molecular structure of SF_4 (sulfur tetrafluoride). SF_4 has a seesaw shape due to the presence of one lone pair on sulfur and four fluorine atoms bonded to it.
2. Determine the polarity of the molecule. Because of the asymmetrical shape and the difference in electronegativity between sulfur and fluorine, SF_4 is a polar molecule, which means it has a permanent dipole moment.
3. Recall the types of intermolecular forces: London dispersion forces (present in all molecules), dipole-dipole interactions (present in polar molecules), and hydrogen bonding (requires H bonded to N, O, or F).
4. Since SF_4 is polar, it exhibits dipole-dipole interactions. Also, all molecules have London dispersion forces, so these are present as well.
5. Check for hydrogen bonding: SF_4 does not have hydrogen atoms bonded to highly electronegative atoms (N, O, or F), so hydrogen bonding is not possible.