Name: how liquids behave on surfaces
Uploaded: 2020-09-24T15:06:49.000Z
Duration: 2 min 57 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Chemistry

Energy

PS.Chm.7.1

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Surface Tension, Capillary Action, and Viscosity

Ever wondered why a yen coin, when carefully placed on water, floats?
Most properties of liquids are dictated by intermolecular forces. The attractive forces between similar molecules in a substance are&#160;called cohesive forces.
In water, the cohesive forces pull interior molecules equally in all directions, resulting in&#160; zero net force on average, while surface molecules experience only a downward pull, which causes the molecules to pack closely together.
The interior molecules are more energetically stable than surface molecules because they experience more cohesion, which lowers their potential energy.
Fluids, therefore, try to reduce their potential energy by minimizing the surface area, creating a surface under tension that behaves like an elastic membrane.
The energy needed to increase a liquid&#8217;s surface area by a unit amount is called its surface tension, which is often measured in joules per meter-squared.
Adhesive forces, in contrast, exist between dissimilar molecules, such as water and glass.
Upon placing a narrow capillary tube in water, the water molecules spread along the tube&#39;s surfaces via adhesion, increasing the liquid&#39;s surface area and drawing the rest of the liqu

surface tension, capillary action, and viscosity

Surface Tension
The various IMFs between identical molecules of a substance are examples of cohesive forces. The molecules within a liquid are surrounded by other molecules and are attracted equally in all directions by the cohesive forces within the liquid. However, the molecules on the surface of a liquid are attracted only by about one-half as many molecules. Because of the unbalanced molecular attractions on the surface molecules, liquids contract to form a shape that minimizes the number of molecules on the surface&#8212;that is, the shape with the minimum surface area. A small drop of liquid tends to assume a spherical shape. This is because the ratio of surface area to volume is at a minimum in a sphere. Larger drops are more greatly affected by gravity, air resistance, surface interactions, and so on, and as a result, are less spherical.
Surface tension is defined as the energy required to increase the surface area of a liquid or the force required to increase the length of a liquid surface by a given amount. This property results from the cohesive forces between molecules at the surface of a liquid, and it causes the surface of a liquid to behave like a stretched rubber membrane. Among common liquids, water exhibits a distinctly high surface tension due to strong hydrogen bonding between its molecules. As a result of this high surface tension, the surface of water represents a relatively &#8220;tough skin&#8221; that can withstand considerable force without breaking. A steel needle carefully placed on water will float. Some insects, even though they are denser than water, move on its surface because they are supported by the surface tension.
Adhesive and Cohesive Forces
The IMFs of attraction between two different molecules are called adhesive forces. Consider what happens when water comes into contact with some surface. If the adhesive forces between water molecules and the molecules of the surface are weak compared to the cohesive forces between the water molecules, the water does not &#8220;wet&#8221; the surface. For example, water does not wet waxed surfaces or many plastics such as polyethylene. Water droplets form on these surfaces because the cohesive forces within the drops are greater than the adhesive forces between the water and the plastic. Water spreads out on glass because the adhesive force between water and glass is greater than the cohesive forces within the water. When water is confined in a glass tube, its meniscus (surface) has a concave shape because the water wets the glass and creeps up the side of the tube. On the other hand, the cohesive forces between mercury atoms are much greater than the adhesive forces between mercury and glass. Mercury, therefore, does not wet glass, and it forms a convex meniscus when confined in a tube because the cohesive forces within the mercury tend to draw it into a drop.
Capillary Action
If one end of a paper towel is placed in spilled wine, the liquid wicks up the paper towel. A similar process occurs in a cloth towel when you use it to dry off after a shower. These are examples of capillary action&#8212;when a liquid flows within a porous material due to the attraction of the liquid molecules to the surface of the material and to other liquid molecules. The adhesive forces between the liquid and the porous material, combined with the cohesive forces within the liquid, may be strong enough to move the liquid upward against gravity.
Towels soak up liquids like water because the fibers of a towel are made of molecules that are attracted to water molecules. Most cloth towels are made of cotton, and paper towels are generally made from paper pulp. Both consist of long molecules of cellulose that contain many &#8722;OH groups. Water molecules are attracted to these &#8722;OH groups and form hydrogen bonds with them, which draws the H2O molecules up the cellulose molecules. The water molecules are also attracted to each other, so large amounts of water are drawn up the cellulose fibers.
Capillary action can also occur when one end of a small diameter tube is immersed in a liquid. If the liquid molecules are strongly attracted to the tube molecules, the liquid creeps up the inside of the tube until the weight of the liquid and the adhesive forces are in balance. The smaller the diameter of the tube is, the higher the liquid climbs.
Viscosity
When you pour a glass of water or fill a car with gasoline, the water and gasoline flow freely. But when you pour syrup on pancakes or add oil to a car engine, the syrup and motor oil do not flow as readily. The viscosity of a liquid is a measure of its resistance to flow. Water, gasoline, and other liquids that flow freely have a low viscosity. Honey, syrup, motor oil, and other liquids that do not flow freely have higher viscosities. We can measure viscosity by measuring the rate at which a metal ball falls through a liquid (the ball falls more slowly through a more viscous liquid) or by measuring the rate at which a liquid flows through a narrow tube (more viscous liquids flow more slowly).
The IMFs between the molecules of a liquid, the size and shape of the molecules, and the temperature determine how easily a liquid flows. The more structurally complex the molecule, the stronger the IMFs between them and the more difficult it is for them to move past each other. Liquids with these molecules are more viscous. As the temperature increases, the molecules move more rapidly and their kinetic energies are better able to overcome the forces that hold them together; thus, the viscosity of the liquid decreases.
This text is adapted from<a href="https://openstax.org/books/chemistry-2e/pages/10-2-properties-of-liquids"> Openstax, Chemistry 2e, Section 10.2: Properties of Liquids</a>.

Surface Tension
The various IMFs between identical molecules of a substance are examples of cohesive forces. The molecules within a liquid are surrounded ...

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JoVE Core

Liquids, Solids, and Intermolecular Forces

KEY TERMS AND CONCEPTS

how liquids behave on surfaces

Liquids behave in different ways on surfaces because of surface tension, adhesive forces, capillary action, and viscosity. These properties help explain why some liquids bead up, some spread out, and some flow more easily than others.

Surface tension comes from cohesive forces, which are the attractions between identical molecules. Molecules inside a liquid are pulled equally in all directions, but molecules at the surface are pulled by fewer neighbors. That imbalance makes the liquid contract into the shape with the least surface area. Small drops tend to be spherical because a sphere has the smallest surface area compared with its volume. Larger drops are less spherical because gravity, air resistance, and surface interactions affect them more. Surface tension is the energy needed to increase a liquid’s surface area, or the force needed to stretch its surface. Water has especially high surface tension because hydrogen bonding between water molecules is strong. That is why a carefully placed steel needle can float, and why some insects can move on water without breaking the surface.

Adhesive forces are the attractions between different molecules. When water touches a surface, the result depends on whether adhesion to the surface is stronger or weaker than cohesion within the water. Water does not wet waxed surfaces or many plastics such as polyethylene because the water molecules attract each other more strongly than they attract the surface. On glass, water spreads out because the attraction between water and glass is stronger than the water-to-water attraction. This is also why water in a glass tube forms a concave meniscus, or curved surface, as it climbs the sides. Mercury behaves differently. The attraction between mercury atoms is stronger than the attraction between mercury and glass, so mercury does not wet glass and forms a convex meniscus.

Capillary action is the movement of a liquid through a porous material or a narrow tube. It happens because the liquid is attracted both to the material and to other liquid molecules. Paper towels and cloth towels absorb spilled wine or shower water because their fibers pull water upward against gravity. Most cloth towels are made of cotton, and paper towels are made from paper pulp. Both contain cellulose, a long molecule with many -OH groups. Water molecules form hydrogen bonds with these groups, which helps draw the water up the fibers. Capillary action also occurs in small tubes. When a liquid strongly attracts the tube walls, it creeps upward until the weight of the liquid balances the adhesive force. The smaller the tube diameter, the higher the liquid rises.

Viscosity is a liquid’s resistance to flow. Water and gasoline have low viscosity because they flow freely. Honey, syrup, and motor oil have higher viscosity because they flow more slowly. Viscosity can be measured by timing how fast a metal ball falls through a liquid or how quickly a liquid moves through a narrow tube. Liquids with stronger intermolecular forces, larger molecules, or more complex shapes are usually more viscous because their particles move past each other less easily. Temperature also matters. As temperature increases, molecules move faster, overcome attractive forces more easily, and the viscosity decreases.

How Liquids Behave on Surfaces

molecular comparison of gases, liquids, and solids

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How Intermolecular Forces Shape States

Intermolecular forces and particle motion shape the states of matter: solids, liquids, and gases. In a solid, particles are tightly packed and often arranged in a regular pattern. A solid has a fixed shape, and its particles vibrate in place rather than flowing past one another. In a liquid, particles stay close together but do not have a regular arrangement. Liquids have no fixed shape, yet their particles move past each other while remaining in contact. That is why liquids can flow and take...

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Liquids behave in different ways on surfaces because of surface tension, adhesive forces, capillary action, and viscosity. These properties help explain why some liquids bead up, some spread out, and some flow more easily than others. Surface tension comes from cohesive forces, which are the attractions between identical molecules. Molecules inside a liquid are pulled equally in all directions, but molecules at the surface are pulled by fewer neighbors. That imbalance makes the liquid contract...

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Explore surface tension, adhesion, capillary action, and viscosity in liquids. See why water beads, towels absorb spills, and some liquids flow more slowly.

How Liquids Behave on Surfaces | JoVE K12

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How Liquids Behave on Surfaces

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