To determine which compound exhibits the weakest overall intermolecular forces, we need to analyze the types of intermolecular forces present in each compound. The possible intermolecular forces can include London dispersion forces, dipole-dipole interactions, and hydrogen bonds. Here’s a step-by-step analysis for each compound:
1. [tex]\( \text{C}_4\text{H}_3\text{OH} \)[/tex]:
- This compound contains a hydroxyl group ([tex]\(-OH\)[/tex]) which can participate in hydrogen bonding.
- Hydrogen bonding is a strong type of intermolecular force, stronger than both dipole-dipole interactions and London dispersion forces.
2. [tex]\( \text{C}_2\text{H}_3\text{O} \)[/tex]:
- This compound likely has a structure that allows for dipole-dipole interactions due to the presence of an electronegative oxygen atom.
- Dipole-dipole interactions are intermediate in strength, stronger than London dispersion forces but weaker than hydrogen bonds.
3. [tex]\( \text{C}_4\text{H}_{10} \)[/tex] (Butane):
- This compound is a nonpolar molecule, meaning it primarily exhibits London dispersion forces.
- London dispersion forces are the weakest of the three types of intermolecular forces.
Given the analysis:
- [tex]\( \text{C}_4\text{H}_3\text{OH} \)[/tex] exhibits hydrogen bonding (strongest).
- [tex]\( \text{C}_2\text{H}_3\text{O} \)[/tex] exhibits dipole-dipole interactions (intermediate strength).
- [tex]\( \text{C}_4\text{H}_{10} \)[/tex] exhibits London dispersion forces (weakest).
Thus, the compound that exhibits the weakest overall intermolecular forces is [tex]\( \text{C}_4\text{H}_{10} \)[/tex] (Butane).
