1 Surface tension, contact angle and work 

Many commonly occurring phenomena that are observed in systems containing an interface in which one of the phases is a liquid can be understood through the concept of surface tension. Some examples are the rise of liquid in a narrow tube, the fact that drops of liquid tend to be spherical, and the observation that water spreads evenly on some surfaces, while remaining in isolated drops on others. In this chapter, surface tension is defined and we see how it can be used to develop simple theories to explain these experiences.  

1.1 Definition of surface tension

The balloon is only an analogy, but something similar happens at the surfaces of interest to us. At any surface, if the force, F, acting tangentially to the surface and at right angles to an element, δx, of an imaginary line in the surface has a magnitude that is independent of the direction of the element, then the surface tension, γ, is:

                                                                                                                                                                                                                                                      (1.1) 

In words, the surface tension is the force per unit length acting on an imaginary line drawn in the surface. The SI units of surface tension are N /m, although because the N /m is rather large (the surface tension of the air–water interface at room temperature is about 72 mN /m), surface tension is more commonly quoted in mN /m (The C.G.S unit for surface tension is the dyn /cm, where 1 dyn/ cm = 1 mN/ m. This unit is seen in the older literature and is rarely used in current work. )  

An intuitive way to understand the origin of surface tension from a molecular point of view is to consider the forces acting on a molecule at the surface of a liquid compared to those acting on one in the bulk (Figure 1.4). The attractive forces acting on one molecule in the bulk are, when averaged over time, isotropic. That is, there is no net force pulling the molecule in any given direction. A molecule at the surface, however, will feel an unbalanced force due to the relative scarcity of near neighbors in the direction of the gas phase. The result is that there is a tendency for that molecule to be pulled into the bulk, as is the case for every other molecule at the surface. Hence, the origin of the tendency to minimize the area of the surface is clear.  

Fig. 1.4 Forces acting on molecules near a surface.