Surfactants reduce the surface tension of water by adsorbing at the gas-liquid interface, and can also reduce the interfacial tension between oil and water by adsorbing at the liquid interface. Many surfactants can also aggregate into aggregates in bulk solutions.
Vesicles and micelles are both types of aggregates. The concentration at which surfactants begin to form micelles is called the critical micelle concentration or CMC. When micelles form in water, their tails form nuclei that can wrap around oil droplets, while their (ionic/polar) heads form an outer shell that remains in contact with water. Surfactants aggregate in oil, and aggregates refer to reverse micelles. In reverse micelles, the head is in the core and the tail maintains sufficient contact with the oil. Surfactants are usually divided into four categories: anions, cations, non ions, and zwitterions (double electrons). The thermodynamics of surfactant systems is crucial, both theoretically and practically. Because surfactant systems represent a system between ordered and disordered states of matter. Surfactant solutions may contain ordered phases (micelles) and disordered phases (free surfactant molecules and/or ions).
For example, commonly used detergents can improve the permeability of water in soil, but the effect only lasts for a few days (many standard laundry detergents contain certain amounts of chemicals, such as sodium and bromine, which are not suitable for soil because they can damage plants).
Commercial soil wetting agents will continue to be effective for a period of time, but ultimately will be degraded by microorganisms. However, some products can have an impact on the biological cycle of aquatic organisms, so care must be taken to prevent these products from flowing into surface runoff, and excessive products should not be washed away.