On the Comparison of Polarity between Ethyl Acetate and Acetone
On Solvent Polarity in the World
The purpose of exploring the polarity of ethyl acetate and acetone. To understand the difference in polarity between the two, we should analyze them by their molecular structure and properties.

The structure of acetone has a carbonyl group, and its carbonyl carbon is connected to oxygen by a double bond. Oxygen is highly electronegative, causing the electron cloud to bias towards the oxygen atom, making the molecule polar. And the carbonyl group of acetone is methyl on both sides, and the structure is relatively symmetric.

Ethyl acetate, containing an ester group, is composed of carbonyl and ethoxy. Carbonyl is polar, but the presence of ethoxy affects the molecular charge distribution. Oxygen in ethoxy is connected to ethyl, which makes the molecular charge distribution more complex than that of acetone.

The polarity is often judged by the dielectric constant. The higher the dielectric constant, the stronger the polarity. According to various experimental data, the dielectric constant of acetone is relatively high, indicating that its polarity is stronger than that of ethyl acetate.

Furthermore, from the perspective of intermolecular forces, the access force, induction force and dispersion force between polar molecules. Acetone has strong polarity and relatively large intermolecular forces. For example, under the same conditions, the boiling point of acetone is slightly higher than that of ethyl acetate, which also proves that the intermolecular force of acetone is strong and the polarity is large.

In summary, compared with ethyl acetate, the polarity of acetone is stronger. This is of important guiding significance for solvent selection in chemical experiments and industrial production. Only by knowing the difference in polarity can we make good use of the two to achieve the best results.