Surface chemistry studies such phenomena as damping, adhesion, sorption and surface tension.
Surface tension (σ) is defined as energy per unit area, [J/m2], or the force that causes the surface of a liquid to contract [N/m]. Among the pure liquids, Hg has a maximum value of σ. Among the biological fluids, H2O has a maximum value of σ, and dissolved substances may either increase or decrease this constant, forming a new system.
As Gibbs’ energy (G) tends to the minimum (ΔG <0 for the spontaneous process), the surface Gibbs’ energy GS = σ ∙ S → min, and for pure liquids S → min is the only way to decrease free surface energy, that is why liquids form drops. The greater σ — the bigger drop may be formed, thus the number of drops in the certain volume is less. This method is often used to find the value of σ in either pure solvents or solutions including biological fluids and drugs. Surface tension (σ) depends on t°, pressure, the polarity of phases, concentration and nature of solutes (or admixtures). Here is another way to decrease free surface energy (GS): the component with a lesser value of σ is pushed out, onto the surface.
There are three groups of substances by the influence on surface tension (σ):
SAA, surface active agents, or surfactants — decrease σ, being pushed out on the surface (e.g.: alcohols, carboxylic acids, thiols, and so on).
SNA, surface nonactive agents, have no influence on σ (e.g.: sucrose, glucose, and so on).
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