Which is the strongest type of intermolecular force present in CHF_3?

• A. Hydrogen bonding
• B. Ion-dipole interactions
• C. London dispersion forces
• D. Dipole-dipole interactions

Answer: (D)

Verified step by step guidance

1. Identify the molecular structure of CHF_3 (fluoroform). It consists of one carbon atom bonded to one hydrogen atom and three fluorine atoms, creating a polar molecule due to the difference in electronegativity between carbon, hydrogen, and fluorine.
2. Recall the types of intermolecular forces: London dispersion forces (present in all molecules), dipole-dipole interactions (present in polar molecules), hydrogen bonding (a special, stronger type of dipole-dipole interaction involving H bonded to N, O, or F), and ion-dipole interactions (between ions and polar molecules).
3. Determine if hydrogen bonding is possible: For hydrogen bonding, hydrogen must be directly bonded to N, O, or F. In CHF_3, hydrogen is bonded to carbon, so hydrogen bonding is not present.
4. Check for ion-dipole interactions: These require the presence of ions interacting with polar molecules. Since CHF_3 is a neutral molecule and no ions are involved, ion-dipole interactions do not apply.
5. Since CHF_3 is polar (due to the electronegativity difference and molecular geometry), the strongest intermolecular force present is dipole-dipole interactions, which are stronger than London dispersion forces but weaker than hydrogen bonding or ion-dipole interactions.