Cl2 is non polar.So there are london dispersion
London forces are present in chlorine molecules.
Cl2 has a stronger intermolecular forces, London dispersion forces, as there are more electrons in Cl2 than in F2 It is the electrons that cause the instantaneous dipole-induced dipole interactions, more electrons = more dipoles and more easily induced dipoles = more london forces.
Intermolecular because intermolecular forces occur between molecules, not within the same molecule. Specifically the forces are London dispersion forces, due to the interaction of instantaneous dipoles.
Dispersion
CH3OH has an H bond with an oxygen molecule, causing H bonding to be a force. It also has dipole-dipole interaction because it's a polar molecule. Thus, it has all three of the forces (including London dispersion).
London forces are present in chlorine molecules.
Cl2 has a stronger intermolecular forces, London dispersion forces, as there are more electrons in Cl2 than in F2 It is the electrons that cause the instantaneous dipole-induced dipole interactions, more electrons = more dipoles and more easily induced dipoles = more london forces.
In Cl2 (chlorine gas), the strongest intermolecular force (IMF) is London dispersion forces, which are a type of van der Waals force. These forces arise due to temporary dipoles created when the electron distribution around the chlorine molecules fluctuates. Although Cl2 is nonpolar, the presence of these temporary dipoles allows for weak attractions between molecules. Overall, London dispersion forces are the only significant IMFs present in Cl2.
Cl2 is non polar.So there are london bonds.
The only intermolecular forces in this long hydrocarbon will be dispersion forces.
Intermolecular because intermolecular forces occur between molecules, not within the same molecule. Specifically the forces are London dispersion forces, due to the interaction of instantaneous dipoles.
Dispersion
Dipole-Dipole and covalent sigma bond forces.
CH3OH has an H bond with an oxygen molecule, causing H bonding to be a force. It also has dipole-dipole interaction because it's a polar molecule. Thus, it has all three of the forces (including London dispersion).
London dispersion forces
London dispersion forces (instantaneous induced dipole-dipole interactions.)
The intermolecular force in CCl4 is dispersion forces. This occurs when slight variations in electron distribution effect the electron distribution of other molecules. Because CCl4 is non polar, it does not have other intermolecular forces holding the molecules together.