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London dispersion forces are a type of intermolecular force. They are relatively weak. They are also called induce-dipole induce-dipole interactions.
* Present in non-polar molecules
* Due to non-systematic electron distribution where one molecule induces a dipole on another molecule
* This is an important factor in very large molecules
* One factor that affects London dispersion forces is polarizability, the ease with which the electron cloud of an atom can be displaced
Wiki User
∙ 15y ago
Wiki User
∙ 15y agoLiquid methane gas, CH4, would be an example of London Dispersion forces. Methane, is a non-polar molecule (meaning there is no buildup of negative or positive charge anywhere on the molecule), thus, there cannot be ionic (eg. table salt) or dipole-dipole (eg. water, H-Bonding in which is an extreme case of dipole-dipole) attractions. Liquid Bromine (Br2(l)) is another example... Located in period four, it has a lot of electrons, distributions of which around the atom can be distorted. Thus, the main force that keeps Br2 liquid at room temperature is London Dispersion Forces.
Wiki User
∙ 14y agoLondon Dispersion Forces are the weakest intermolecular forces between molecules. Imagine a molecule as a huge mass of protons, electrons and neutrons (that's all they are in different amounts based on what atoms are in the molecule) enclosed in a certain area. Protons are positive. Electrons are negative and neutrons have no discernable charge. When two molecules are put next to eachother, the negative and positive charges can temporarily separate to opposite sides of the "area" of the molecule. They then bond accordingly to other molecules (positive of one is attracted to the negative of the other). They are extremely weak due to the temporary polarization effect wanting to go back to normal.
Wiki User
∙ 12y agoWhen you design soap, the London dispersion forces is what actually grabs the oil molecules because after all, soaps are just lipids.
Wiki User
∙ 10y agoLondon forces in chemistry are called dispersion forces. Every substance has dispersion forces between its particles. These forces are present in all compounds.
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