When comparing the intermolecular forces of attraction between the given substances, ethanoic acid (or acetic acid) has the greatest intermolecular forces. This is primarily due to its ability to form strong hydrogen bonds.
Here’s a brief explanation of each substance:
- Propanone: Also known as acetone, it has dipole-dipole interactions and some Van der Waals forces, but lacks the hydrogen bonding capacity seen in water and ethanoic acid.
- Ethanol: This alcohol also forms hydrogen bonds, which makes its intermolecular forces stronger than those in propanone, but not as strong as those in ethanoic acid.
- Water: Water has very strong hydrogen bonding, which gives it high cohesion and a higher boiling point compared to many other substances. However, ethanoic acid can form two hydrogen bonds per molecule due to its structure, which enhances its intermolecular attractions.
- Ethanoic Acid: Ethanoic acid can donate and accept hydrogen bonds due to its carboxylic group. This dual ability allows it to have stronger intermolecular forces compared to the other substances listed, making it the substance with the greatest intermolecular forces of attraction.
In conclusion, while water and ethanol exhibit significant hydrogen bonding, ethanoic acid’s structure allows it to foster stronger intermolecular interactions, establishing it as the substance with the greatest intermolecular forces of attraction among the four.