Which substance has the greatest intermolecular forces of attraction between molecules? Is it propane ethanol water or ethanolic acid
To be honest about it I don't know the answer to this question. However, based on the size of a water molecule vs the size of the acetic acid molecule, the distances for a hydrogen bond are greater in acetic acid intermolecular (not intramolecular) and as such the water intermolecular bonds would be stronger due to the proximity issues. Please let me know if you find differently.
Among the substances you mentioned, ethanoic acid (also known as acetic acid) has the greatest intermolecular forces of attraction between molecules. Ethanoic acid has strong hydrogen bonding between its molecules, resulting in a high boiling point and greater intermolecular forces compared to the other substances mentioned.
Propane, ethanol, and water also have intermolecular forces, but they primarily rely on London dispersion forces and dipole-dipole interactions, which are generally weaker than hydrogen bonding. Additionally, while ethanol and water can form hydrogen bonds, their intermolecular forces are still not as strong as those in ethanoic acid.
Therefore, in terms of intermolecular forces, ethanoic acid has the strongest attraction between its molecules.
To determine which substance has the greatest intermolecular forces of attraction between molecules, we need to consider the types of intermolecular forces present in each substance.
Propane is a nonpolar molecule and only exhibits London dispersion forces, which arise from temporary fluctuations in electron distribution. While London dispersion forces are relatively weak, they still contribute to intermolecular attractions.
Ethanol is a polar molecule due to the presence of the hydroxyl (-OH) group. In addition to London dispersion forces, ethanol exhibits hydrogen bonding between the hydrogen atom in the hydroxyl group and the oxygen atom of another ethanol molecule. Hydrogen bonds are stronger than London dispersion forces.
Water, a highly polar molecule, also exhibits both London dispersion forces and hydrogen bonding. The presence of two hydrogen atoms in each water molecule allows for multiple hydrogen bonding interactions between adjacent water molecules. Water's strong hydrogen bonding leads to its unique properties, such as high boiling point, surface tension, and specific heat capacity.
Ethanolic acid, or acetic acid, is also a polar molecule with a carboxyl group (-COOH). It exhibits both London dispersion forces and stronger hydrogen bonding due to its polar nature and the presence of the hydrogen and oxygen atoms involved in forming hydrogen bonds.
Considering the intermolecular forces discussed above, we can conclude that ethanolic acid would have the greatest intermolecular forces of attraction between molecules among the given substances, followed by water, ethanol, and propane.