All of the attractive forces between neutral atoms and molecules are known as van der Waals forces, although they are usually referred to more informally as intermolecular attraction. These are the intermolecular forces for the dissolution of many types of gases in a solvent like water. You can view the transcript for Smart materials (1 of 5): Gecko Adhesive fit for Spiderman here (opens in new window). The electronegativity difference between H and O, N, or F is usually more than other polar bonds. As an example of the processes depicted in this figure, consider a sample of water. Intramolecular forces are those within the molecule that keep the molecule together, for example, the bonds between the atoms. Ethane (CH3CH3) has a melting point of 183 C and a boiling point of 89 C. And while a gecko can lift its feet easily as it walks along a surface, if you attempt to pick it up, it sticks to the surface. We need to be careful in extrapolating trends here though, especially if the solute is not a gas, and will take a more detailed look at solutions in chapter 13, where in addition to the solute/solvent interactions described by dipole-induced dipole interactions of polar/nonpolar intermolecular interactions, we will also take into account solute/solute and solvent/solvent interactions. The strongest intermolecular force is hydrogen bonding, which is a particular subset of dipole-dipole interactions that occur when a hydrogen is in close proximity (bound to) a highly electronegative element (namely oxygen, nitrogen, or fluorine). Select all that are TRUE Dipole-Dipole Forces (not including Hydrogen Bonding) Hydrogen Bonding Induced Dipole-Induced Dipole (London Dispersion) Forces Induced Dipole-Dipole Forces. Nonmetals tend to make a covalent bond with each other. For symmetric nonpolar molecules these can form waves as successive instantaneously induced dipoles that in turn induce dipoles on their neighbors, and thus are often called dispersion forces. Molecules with a large \(alpha\) are easy to induce a dipole. This attractive force is called a dipole-dipole attractionthe electrostatic force between the partially positive end of one polar molecule and the partially negative end of another, as illustrated in Figure 8. What is the predominant intermolecular force in ? 21. The temporary dipole that results from the motion of the electrons in an atom can induce a dipole in an adjacent atom and give rise to the London dispersion force. Under appropriate conditions, the attractions between all gas molecules will cause them to form liquids or solids. 1. 11. The intermolecular force is the sum of all the forces between two neighboring molecules. Figure 4 illustrates these different molecular forces. They differ in that the particles of a liquid are confined to the shape of the vessel in which they are placed. At a temperature of 150 K, molecules of both substances would have the same average KE. Which interaction is more important depends on temperature and pressure (see compressibility factor). London forces increase with increasing molecular size. They are incompressible and have similar densities that are both much larger than those of gases. Dispersion forces exist between any two molecules and generally increase as the molecular weight of the molecule increases. 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