What types of intermolecular forces exist in a sample of acetone? (LO 8.8)
(a) Dispersion forces (b) Dispersion forces and dipole–dipole forces (c) Dipole–dipole forces (d) Dispersion forces, dipole–dipole forces, and hydrogen bonding

Verified step by step guidance

1. Identify the molecular structure of acetone: (CH3)2CO.
2. Recognize that acetone has a polar carbonyl group (C=O), which can lead to dipole-dipole interactions.
3. Understand that all molecules exhibit dispersion forces (also known as London dispersion forces).
4. Determine if hydrogen bonding is possible: Acetone does not have hydrogen atoms directly bonded to highly electronegative atoms (N, O, or F), so it cannot form hydrogen bonds.
5. Conclude that the intermolecular forces present in acetone are dispersion forces and dipole-dipole forces.

Key Concepts

Intermolecular Forces

Intermolecular forces are the attractive forces between molecules that influence physical properties such as boiling and melting points. The main types include dispersion forces, dipole-dipole interactions, and hydrogen bonding. Understanding these forces is crucial for predicting how substances behave in different states and conditions.

Dispersion Forces

Dispersion forces, also known as London dispersion forces, are weak intermolecular forces arising from temporary fluctuations in electron density within molecules. These forces are present in all molecules, regardless of polarity, and become more significant in larger, more polarizable molecules. In acetone, dispersion forces contribute to its overall intermolecular interactions.

Dipole-Dipole Forces

Dipole-dipole forces occur between polar molecules that have permanent dipoles due to differences in electronegativity between bonded atoms. In acetone, the presence of a carbonyl group (C=O) creates a dipole, allowing for dipole-dipole interactions with other acetone molecules. These forces are stronger than dispersion forces and significantly affect the physical properties of polar substances.