Dictionary:

diffusion

  (dĭ-fyū'zhən)

1. The process of diffusing or the condition of being diffused.
2. Needless profusion of words; prolixity.
3. Physics.
   1. The scattering of incident light by reflection from a rough surface.
   2. The transmission of light through a translucent material.
   3. The spontaneous intermingling of the particles of two or more substances as a result of random thermal motion.
4. The spread of linguistic or cultural practices or innovations within a community or from one community to another.

The transport of matter from one point to another by random molecular motions. It occurs in gases, liquids, and solids.

Diffusion plays a key role in processes as diverse as permeation through membranes, evaporation of liquids, dyeing textile fibers, drying timber, doping silicon wafers to make semiconductors, and transporting of thermal neutrons in nuclear power reactors. Rates of important chemical reactions are limited by how fast diffusion can bring reactants together or deliver them to reaction sites on enzymes or catalysts. The forces between molecules and molecular sizes and shapes can be studied by making diffusion measurements. See also Evaporation.

Molecules in fluids (gases and liquids) are constantly moving. Even in still air, for example, nitrogen and oxygen molecules ricochet off each other at bullet speeds. Molecular diffusion is easily demonstrated by pouring a layer of water over a layer of ink in a narrow glass tube. The boundary between the ink and water is sharp at first, but it slowly blurs as the ink diffuses upward into the clear water. Eventually, the ink spreads evenly along the tube without any help from stirring.

Gases

A number of techniques are used to measure diffusion in gases. In a two-bulb experiment, two vessels of gas are connected by a narrow tube through which diffusion occurs. Diffusion is followed by measuring the subsequent changes in the composition of gas in each vessel. Excellent results are also obtained by placing a lighter gas mixture on top of a denser gas mixture in a vertical tube and then measuring the composition along the tube after a timed interval.

Rates of diffusion in gases increase with the temperature (T) approximately as T^3/2 and are inversely proportional to the pressure. The interdiffusion coefficients of gas mixtures are almost independent of the composition.

Kinetic theory shows that the self-diffusion coefficient of a pure gas is inversely proportional to both the square root of the molecular weight and the square of the molecular diameter. Interdiffusion coefficients for pairs of gases can be estimated by taking averages of the molecular weights and collision diameters. Kinetic-theory predictions are accurate to about 5% at pressures up to 10 atm (1 megapascal). Theories which take into account the forces between molecules are more accurate, especially for dense gases.

Liquids

The most accurate diffusion measurements on liquids are made by layering a solution over a denser solution and then using optical methods to follow the changes in refractive index along the column of solution. Excellent results are also obtained with cells in which diffusion occurs between two solution compartments through a porous diaphragm. Many other reliable experimental techniques have been devised.

Room-temperature liquids usually have diffusion coefficients in the range 0.5–5 × 10⁻⁵ cm² s⁻¹. Diffusion in liquids, unlike diffusion in gases, is sensitive to changes in composition but relatively insensitive to changes in pressure. Diffusion of high-viscosity, syrupy liquids and macromolecules is slower. The diffusion coefficient of aqueous serum albumin, a protein of molecular weight 60,000 atomic mass units, is only 0.06 × 10⁻⁵ cm² s⁻¹ at 25°C (77°F).

When solute molecules diffuse through a solution, solvent molecules must be pushed out of the way. For this reason, liquid-phase interdiffusion coefficients are inversely proportional to both the viscosity of the solvent and the effective radius of the solute molecules. Accurate theories of diffusion in liquids are still under development.

Solids

Diffusion in solids is an important topic of physical metallurgy and materials science since diffusion processes are ubiquitous in solid matter at elevated temperatures. They play a key role in the kinetics of many microstructural changes that occur during the processing of metals, alloys, ceramics, semiconductors, glasses, and polymers. Typical examples of such changes include nucleation of new phases, diffusive phase transformations, precipitation and dissolution of a second phase, recrystallization, high-temperature creep, and thermal oxidation. Direct technological applications concern diffusion doping during the fabrication of microelectronic devices, solid electrolytes for battery and fuel cells, surface hardening of steels through carburization or nitridation, diffusion bonding, and sintering. See also Fuel cell; Phase transitions.

The atomic mechanisms of diffusion are closely connected with defects in solids. Point defects such as vacancies and interstitials are the simplest defects and often mediate diffusion in an otherwise perfect crystal. Dislocations, grain boundaries, phase boundaries, and free surfaces are other types of defects in a crystalline solid. They can act as diffusion short circuits because the mobility of atoms along such defects is usually much higher than in the lattice.

A semiconductor manufacturing process that infuses tiny quantities of impurities into a base material, such as silicon, to change its electrical characteristics. See chip.

Diffusion Process

This diagram shows the masking, etching and diffusion stages that build the tiny sublayers in a transistor.

Process by which a new product or idea attracts the attention and interest of a market and is gradually adopted by the many individuals making up that market. Unlike individual adoption decisions, diffusion is influenced by communication about a product between an ever-widening group of consumers and is affected by the social dynamics of the group. See also adoption process; innovation; early adopter; innovator.

The name applied to a physical process by which individual particles move randomly, within a fluid, from areas of high concentration to lower concentration until the particles are evenly distributed throughout the space. The particles referred to can be molecules or ions and the fluid can be either gaseous or liquid. For example, a person wearing perfume can be noticed on entering a room because molecules of the odiferous substances contained within the perfume diffuse in the air and are detected by the nose. Similarly, a drop of dye dropped into a glass of water will eventually colour the whole volume as the molecules of dye diffuse evenly throughout the volume. Because of thermal motion and vibration, a molecule, ion, or small particle undergoes 10¹³ to 10¹⁵ collisions per second with molecules of the fluid. The particle is said to undergo a random walk, in which the result of a particular collision is independent of the effects of previous collisions. The statistical consequence of this is that the displacement of a particle from its original position will depend on the elapsed time. Where the diffusing particles are at high concentration, many collisions will be between the diffusing species, so that they will move away from each other, thus creating a flux from high concentration to low until the concentration is even throughout the volume. Diffusion is influenced by many factors, such as viscosity and electric charge. Thus diffusion in treacle will be slower than diffusion in water, and particles carrying the same charge will exert mutual repulsion.

Diffusion is an important process for bodily function. Important substances, such as oxygen and carbon dioxide, not only need to diffuse within a particular fluid volume but need to diffuse from one bodily compartment to another across barriers, where generally diffusion will be slower than within a fluid. Consider the position in the lungs; oxygen from the air has to diffuse across the walls of the alveoli and of the capillaries within the lungs to reach the blood, and then across the walls of the red cells to reach the haemoglobin. Fortunately it combines with the haemoglobin to form oxyhaemoglobin, thus maintaining a steep concentration gradient. At the same time carbon dioxide, released from the venous blood, needs to diffuse in the opposite direction, down its concentration gradient, into the lungs, in order to be exhaled. As the transit time of blood in the lungs is just a few seconds, the diffusive process needs to be rapid. (If, for example, the lungs are filled with thick, viscid mucus, as in bronchiectasis or cystic fibrosis, then the diffusive process is impaired and full oxygenation will not occur). Conversely, when oxygenated blood arrives at the tissues the conditions are such that oxygen is released and needs to diffuse into the cells to maintain tissue respiration, whilst carbon dioxide, a product of tissue respiration, needs to be loaded into the blood for conveyance back to the lungs.

Diffusion is similarly important in the absorptive processes in the gut. The purpose of digestion is to break down complex molecules into simple ones such as sugars, fats, and peptides. The lining of the gut wall has many specialized transporters to take the breakdown products into the cells and to transfer them to the blood, for delivery to tissues where they can be used as a source of energy, stored, or used for growth and repair. However, to arrive at the transporters the products of digestion need to diffuse from the gut contents, through the aqueous stationary layer closest to the lining of the gut, to reach the transporters. Diffusion therefore is a universally important process affecting every aspect of living tissue. A single living cell is a hive of activity. Substances produced within the cell which are important for its normal functioning may be produced at one site but then interact with another part of the cell, which they reach by diffusion, moving from high concentration to low by way of thermal motion, an inherent physical property.

— Alan W. Cuthbert

noun

Words or the use of words in excess of those needed for clarity or precision: diffuseness, long-windedness, pleonasm, prolixity, redundancy, verbiage, verboseness, verbosity, windiness, wordage, wordiness. See excess/insufficiency/enough, style/good style/bad style, words.

Definition: spread; wide distribution
Antonyms: centralization, collection, concentration

A property of ions or molecules of a solute that permits them to pass through a membrane or to intermingle by rapid or gradual permeation with the molecules of a solvent.

The widespread dispersal of an innovation from a centre or centres. This innovation may be anything from an epidemic disease to a political belief, or even the wearing of reversed baseball caps.

T. Hägerstrand's model of diffusion (1968) implies the existence of a mean information field which regulates the flows of information around a regional system. These flows are moderated by barriers which can obstruct the evolution of information into innovation, and thus mould the diffusion wave; the ripple of innovation which spreads from one location to another.

Various categories of diffusion have been recognized: expansion diffusion is the spread of a factor from a centre with the concentration of the things being diffused also remaining, and possibly intensifying, at the point of origin. One example is the spread of girls' public day schools in the nineteenth century, which started in London. As new schools developed further and further away from London, new schools also opened in the capital. Relocation diffusion similarly spreads from a centre but the innovation moves outwards, leaving the centre. An example of this is the movement of a bush fire, which has burned out at the origin but continues to spread at the periphery. Hierarchic diffusion passes through a regular sequence of orders as when an innovation in a metropolis spreads out to cities, then towns, and finally to villages. A good example is the introduction of video hire shops. The order of the diffusion may also be based on class—the spread of wine-drinking in Britain is a good example. The innovation may spread up a hierarchy, but cascade diffusion is a form of hierarchic diffusion which only moves down an order or hierarchy.

The Hägerstrand model has shortcomings: it does not explain why some adopt an innovation and others do not, and it is based on the notion of a uniform cognitive region through which innovation diffuses, whereas access to information is socially structured.

Recent work on diffusion has focused on the transmission of epidemics; the diffusion of HIV/AIDS, for example, seems to depend on: distance from a transmission pathway; access to travel facilities; and the propensity to travel. See spatial diffusion analysis.

For more information on diffusion, visit Britannica.com.

1. The net movement of molecules of a fluid from a high concentration to a low concentration. Diffusion is a passive process resulting from the random movement of molecules as a result of their kinetic energy. Gaseous exchange in the lungs and tissues takes place by diffusion through biological membranes. The rate of diffusion depends on the concentration gradient, diffusion distance, and the surface area and properties of the membrane.

2. The spread of cultural traits, such as language, technological ideas, or social practices from one society to another.

The spreading of atoms or molecules of one substance through those of another, especially into liquids or gases.

1. the state or process of being widely spread.
2. the spontaneous mixing of the molecules or ions of two or more substances resulting from random thermal motion; its rate is proportional to the concentrations of the substances and it increases with the temperature.
In the body fluids the molecules of water, gases, and the ions of substances in solution are in constant motion. As each molecule moves about, it bounces off other molecules and loses some of its energy to each molecule it hits, but at the same time it gains energy from the molecules that collide with it.
The rate of diffusion is influenced by the size of the molecules; larger molecules move less rapidly, because they require more energy to move about. Molecules of a solution of higher concentration move more rapidly toward those of a solution of lesser concentration; in other words, the rate of movement from higher to lower concentration is greater than the movement in the opposite direction.

• d. coefficient — the number of milliliters of a gas that will diffuse at a distance of 0.001 mm over a square centimeter surface per minute, at 1 atmosphere of pressure. The diffusion coefficient for any given gas is proportional to the solubility and molecular weight of the gas. The diffusion coefficient for oxygen is 1.0, for carbon dioxide it is 20.3, and for nitrogen it is 0.53. The diffusion capacity of a gas varies directly with the diffusion coefficient.
• facilitated d. — mechanisms in intestinal absorption which assist the passage of those products of digestion, which cannot occur by simple diffusion, across the intestinal cell membranes. They include a carrier mechanism involving proteins, and active transport which provides energy from the breakdown of high-energy phosphate bonds.
• Fick's first law of d. — see fick's first law of diffusion.
• d. hypoxia — a transient hypoxic episode after the cessation of nitrous oxide anesthesia if air is inhaled instead of pure oxygen; caused by the rapid diffusion of nitrous oxide out into the alveoli diluting the oxygen that is there.

Tendency of conduction band electrons to wander across a pn junction to combine with valence band holes.

This article is about the physical mechanism of diffusion. For alternative meanings, see diffusion (disambiguation).

Diffusion is the net movement of particles from an area of high concentration to an area of low concentration. For example, diffusing molecules will move randomly between areas of high and low concentration but because there are more molecules in the high concentration region, more molecules will leave the high concentration region than the low concentration one. Therefore, there will be a net movement of molecules from high to low concentration. Initially, a concentration gradient—a smooth decrease in concentration from high to low—will form between the two regions. As time progresses, the gradient will grow increasingly shallow until the concentrations are equalized.

Diffusion is a spontaneous process (more familiarly known as a "passive" form of transport, rather than "active"); it is simply the statistical outcome of random motion. Diffusion increases entropy, decreasing Gibbs free energy, and therefore is thermodynamically favorable. Diffusion operates within the boundaries of the Second Law of Thermodynamics because it demonstrates nature's tendency to wind down, as evidenced by increasing entropy.^[1]

The diffusion equation provides a mathematical description of diffusion. This equation is derived from Fick's law, which states that the net movement of diffusing substance per unit area of section (the flux) is proportional to the concentration gradient (how steeply the concentration changes in space), and is toward lower concentration. (Thus if the concentration is uniform there will be no net motion.) The constant of proportionality is the diffusion coefficient, which depends on the diffusing species and the material through which diffusion occurs. Fick's law is an assumption that may not hold for a given diffusive system (e.g., the diffusion may depend on concentration in addition to concentration gradient), in which case the motion would not be described by the normal (simple, Fickian) diffusion equation. An analogous statement of Fick's law, for heat instead of concentration, is Fourier's law.

Diffusion can also be described using discrete quantities (the diffusion equation has derivatives and thus applies to continuous quantities). A common model of discrete diffusion is the random walk. A random walk model is connected to the diffusion equation by considering an infinite number of random walkers starting from a non-uniform configuration, where the evolution of the concentration is described by the diffusion equation.

Diffusion is often important in systems experiencing an applied force. In a conducting material, the net motion of electrons in an electrical field quickly reaches a terminal velocity (resulting in a steady current described by Ohm's law) because of the thermal (diffusive) motions of atoms. The Einstein relation relates the diffusion coefficient to the mobility of particles.

In cell biology, diffusion is a main form of transport within cells and across cell membranes.

Types of diffusion

The spreading of any quantity that can be described by the diffusion equation or a random walk model (e.g. concentration, heat, momentum, ideas, price) can be called diffusion. Some of the most important examples are listed below.

• Atomic diffusion
• Brownian motion, for example of a single particle in a solvent
• Collective diffusion, the diffusion of a large number of (possibly interacting) particles
• Effusion of a gas through small holes.
• Electron diffusion, resulting in electric current
• Gaseous diffusion, used for isotope separation
• Heat flow
• Itō diffusion
• Knudsen diffusion
• Momentum diffusion, ex. the diffusion of the hydrodynamic velocity field
• Osmosis
• Photon diffusion
• Reverse diffusion
• Self-diffusion

Metabolism and respiration rely in part upon diffusion in addition to bulk or active processes. For example, in the alveoli of mammalian lungs, due to differences in partial pressures across the alveolar-capillary membrane, oxygen diffuses into the blood and carbon dioxide diffuses out. Lungs contain a large surface area to facilitate this gas exchange process.

An experiment to demonstrate diffusion

Diffusion is easy to observe, but care must be taken to avoid a mixture of diffusion and other transport processes.

It can be demonstrated with a wide glass tube, two corks, some cotton wool soaked in ammonia solution and some red litmus paper. By corking the two ends of the wide glass tube and plugging the wet cotton wool with one of the corks, and the litmus paper can be hung with a thread within the tube. It will be observed that the red litmus papers turn blue.

This is because the ammonia molecules travel by diffusion from the higher concentration in the cotton wool to the lower concentration in the rest of the glass tube. As the ammonia solution is alkaline, the red litmus papers turn blue. By changing the concentration of ammonia, the rate of color change of the litmus papers can be changed.

References

1. ^ Biddle, Verne, and Gregory Parker. Chemistry: Precision and Design. Pensacola: A Beka Book, 2000. p109.

See also

Wikibooks' [[wikibooks:|]] has more about this subject:

Constructing school science lab equipment/Apparatus for demonstrating osmosis

• Bohm diffusion
• Brownian motion
• Collective diffusion
• Diffusion equation
• Diffusion equilibrium
• Diffusion MRI
• Fick's law of diffusion
• Isotope separation
• Mass transfer
• Osmosis
• Transport phenomena
• Local time (mathematics)

External links

• Some pictures that display diffusion and osmosis
• An animation describing diffusion.
• A tutorial on the theory behind and solution of the Diffusion Equation.

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