Question

aspirin is a crystalline molecular solid. shown below is a lewis structure for aspirin, together with a representation of six aspirin molecules as they are arranged in the crystalline solid. which of the following intermolecular forces are present in aspirin. the question asks about all of the possible intermolecular forces, not just the strongest one. when aspirin melts the intermolecular forces between the aspirin molecules need to be broken. o hydrogen bonding only o hydrogen bonding and dipole - dipole forces o hydrogen bonding, dipole - dipole forces and london dispersion forces o hydrogen bonding and london dispersion forces

Explanation:

Step1: Analyze hydrogen - bonding

Aspirin has polar O - H and C=O groups. Hydrogen - bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (N, O, or F) and is attracted to another electronegative atom. In aspirin, hydrogen - bonding can occur between the O - H group of one aspirin molecule and the C=O or other electronegative O atoms of neighboring molecules.

Step2: Analyze dipole - dipole forces

Aspirin is a polar molecule due to the presence of functional groups like the carboxyl group ( - COOH) and the ester group ( - COO - ). Dipole - dipole forces act between polar molecules, where the positive end of one dipole is attracted to the negative end of another dipole.

Step3: Analyze London dispersion forces

London dispersion forces are present in all molecules, including aspirin. These forces are due to temporary fluctuations in electron distribution, creating instantaneous dipoles. Larger molecules with more electrons generally have stronger London dispersion forces. Since aspirin has a relatively large molecular structure, it has London dispersion forces.

Answer:

Hydrogen bonding, dipole - dipole forces and London dispersion forces