Question

below is a lewis structure for a compound: lewis structure image based on the structure, select all of the intermolecular forces that would be present between molecules. hint: you have to consider polarity, ☐ dipole-dipole interactions ☐ hydrogen bonding ☐ ion-dipole interactions ☐ london dispersion forces

Explanation:

1. Dipole - dipole interactions: The compound has polar bonds (e.g., C = O and C - O bonds) and a polar molecular structure overall, so dipole - dipole interactions occur between polar molecules.
2. London dispersion forces: All molecules, regardless of polarity, have London dispersion forces due to temporary fluctuations in electron density.
3. Hydrogen bonding: For hydrogen bonding, a hydrogen atom must be bonded to a highly electronegative atom (F, O, N) and interact with another electronegative atom. In this structure, the hydrogens are bonded to carbon, not to O (the O is bonded to C), so no hydrogen bonding.
4. Ion - dipole interactions: The compound is a neutral molecule, not an ion, so ion - dipole interactions (which require an ion and a polar molecule) do not occur.

Answer:

Dipole - dipole interactions, London dispersion forces