Ad
related to: he intermolecular forces
Search results
Results From The WOW.Com Content Network
The attractive force draws molecules closer together and gives a real gas a tendency to occupy a smaller volume than an ideal gas. Which interaction is more important depends on temperature and pressure (see compressibility factor). In a gas, the distances between molecules are generally large, so intermolecular forces have only a small effect.
London dispersion forces (LDF, also known as dispersion forces, London forces, instantaneous dipole–induced dipole forces, fluctuating induced dipole bonds [1] or loosely as van der Waals forces) are a type of intermolecular force acting between atoms and molecules that are normally electrically symmetric; that is, the electrons are ...
Fritz Wolfgang London (March 7, 1900 – March 30, 1954) was a German born physicist and professor at Duke University.His fundamental contributions to the theories of chemical bonding and of intermolecular forces (London dispersion forces) are today considered classic and are discussed in standard textbooks of physical chemistry.
Intermolecular forces are experienced by molecules when they are within physical proximity of one another. [20] [21] These forces are very important for properly modeling molecular systems, as to accurately predict the microscopic behavior of molecules in any system, and therefore, are necessary for accurately predicting the physical properties ...
The ideal gas model tends to fail at lower temperatures or higher pressures, when intermolecular forces and molecular size becomes important. It also fails for most heavy gases, such as many refrigerants, [2] and for gases with strong intermolecular forces, notably water vapor. At high pressures, the volume of a real gas is often considerably ...
Since he was one of the first to postulate an intermolecular force, however rudimentary, such a force is now sometimes called a Van der Waals force. A second major discovery was the 1880 the law of corresponding states, which showed that the Van der Waals equation of state can be expressed as a simple function of the critical pressure, critical ...
Deviations of the compressibility factor, Z, from unity are due to attractive and repulsive intermolecular forces. At a given temperature and pressure, repulsive forces tend to make the volume larger than for an ideal gas; when these forces dominate Z is greater than unity. When attractive forces dominate, Z is less than unity.
Pages in category "Intermolecular forces" The following 44 pages are in this category, out of 44 total. This list may not reflect recent changes. A. Adhesion;