London Dispersion Forces
ionic
Intermolecular forces are of the type(1) hydrogen bonds (2) dipole-dipole attractions (3) dispersion forces (van der Waals, etc.)
Dispersion forces (London dispersion forces) are generally the weakest type of intermolecular force. These forces are caused by temporary fluctuations in electron distribution around atoms or molecules, leading to weak attractions between them.
Bonding affects intermolecular forces by influencing the strength of attractions between molecules. Covalent bonds within molecules contribute to intramolecular forces, while intermolecular forces, such as hydrogen bonding or van der Waals forces, occur between molecules. The type and strength of bonding within a molecule can impact the overall intermolecular forces affecting its physical properties.
Aluminum primarily exhibits metallic bonding, which is characterized by a "sea of electrons" that allows for conductivity and malleability. While aluminum itself doesn't have significant van der Waals forces or hydrogen bonding, it can form oxide layers that introduce some ionic character through interactions with oxygen. However, in its metallic state, the dominant intermolecular forces are those associated with metallic bonding.
Intramolecular forces are not intermolecular forces !
Chlorine exhibits London dispersion forces as its dominant intermolecular force. This is due to its nonpolar covalent bonding and symmetrical molecular structure that results in temporary dipoles between molecules.
ionic
Nitrogen fluoride (NF3) is a polar molecule, so the dominant intermolecular forces present are dipole-dipole interactions. Additionally, NF3 can also exhibit weak van der Waals dispersion forces between its molecules.
London forces are present in chlorine molecules.
not an (F,O,N) atom therefore it has no H bond, it has no dipole dipole interactions, plus London forces are weak. Which is why it has a a very low critical temperature.
Intermolecular forces are of the type(1) hydrogen bonds (2) dipole-dipole attractions (3) dispersion forces (van der Waals, etc.)
Dispersion forces (London dispersion forces) are generally the weakest type of intermolecular force. These forces are caused by temporary fluctuations in electron distribution around atoms or molecules, leading to weak attractions between them.
Bonding affects intermolecular forces by influencing the strength of attractions between molecules. Covalent bonds within molecules contribute to intramolecular forces, while intermolecular forces, such as hydrogen bonding or van der Waals forces, occur between molecules. The type and strength of bonding within a molecule can impact the overall intermolecular forces affecting its physical properties.
Hydrocarbons typically exhibit London dispersion forces as the predominant intermolecular force due to the presence of nonpolar carbon-carbon and carbon-hydrogen bonds. Additionally, larger hydrocarbons can also exhibit weak van der Waals forces. Overall, the intermolecular forces in hydrocarbons are relatively weak compared to compounds with polar covalent bonds.
dipole-dipole attractions
hydrogen bonds