The polarity of ethyl acetate and water
is related to its molecular structure and charge distribution, and has a key impact on everything in chemistry, such as dissolution and reaction. The polarity of ethyl acetate and water can be explained by the difference in its properties and its role in various chemical processes.

For water, its molecules have a V-shaped structure, the oxygen atom has strong electronegativity, and the charge distribution between hydrogen and oxygen bonds is uneven. One side of the oxygen atom is rich in electrons, which is negative, and one side of the hydrogen atom lacks electrons, which is positive, so it becomes a significant polar molecule. This results in the formation of hydrogen bonds between polar water molecules, which increases the intermolecular forces, such as higher boiling points and greater surface tension.

In contrast, ethyl acetate, its structure contains ester groups, although it also has a certain polarity, but compared with water, the carbon and hydrogen chain part of its molecule accounts for a larger proportion. The electronegativity difference between hydrocarbons is small, the charge distribution is relatively uniform, and the polar effect of ester groups is limited. Therefore, in general, the polarity of ethyl acetate is weaker than that of water.

In practical applications, due to the difference in polarity between the two, its solubility is different. Water is a polar solvent and can dissolve many polar substances, such as salts, alcohols, etc.; while ethyl acetate, as a weak polar solvent, is more likely to dissolve non-polar or weakly polar substances, such as some oils, organic dyes, etc. From this perspective, the polarity of ethyl acetate is indeed not as good as that of water. This difference is a basic understanding in the field of chemistry, and it is an important consideration in terms of material separation, purification, and choice of reaction conditions. It helps us to understand chemical phenomena in depth and optimize chemical processes.