The predominant intermolecular force in ammonia (NH3) is hydrogen bonding. Hydrogen bonding occurs between the hydrogen atom of one ammonia molecule and the lone pair of electrons on the nitrogen atom of another ammonia molecule. This results in relatively strong interactions between the molecules.
The predominant intermolecular force in methane is London dispersion forces, in ammonia it is hydrogen bonding, in nitrogen trifluoride it is dipole-dipole interactions.
Dipole forces and London forces are present between these molecules.
Ammonia has a higher boiling point than phosphine because ammonia molecules are held together by stronger hydrogen bonds, compared to the weaker van der Waals forces between phosphine molecules. This results in a higher amount of energy needed to overcome the intermolecular forces and cause the substance to boil.
AlH3 alane is a covalent solid and is a giant molecule, so no intermolecular forces will be present. Planar AlH3 molecules have been isolated at very low temperatures. AlH3 molecules would be predicted to have no dipole moment due to their shape. The only intermolecular forces would be London dispersion forces.
Water (H2O) has stronger intermolecular forces than ammonia (NH3) due to hydrogen bonding in water molecules. Hydrogen bonding is a type of intermolecular force that is stronger than the dipole-dipole interactions present in ammonia molecules.
The strongest intermolecular force present in ibuprofen is dipole-dipole interactions. Ibuprofen contains polar covalent bonds due to the differences in electronegativity between the atoms, leading to the formation of partial positive and negative charges. These partial charges allow ibuprofen molecules to attract each other through dipole-dipole interactions.
The strongest intermolecular force in CCl2H2 (dichloromethane) is dipole-dipole interactions. This is because dichloromethane has polar bonds due to the difference in electronegativity between carbon and chlorine, resulting in a permanent dipole moment.
Because there is the present of intermolecular force and intramolecular force
The predominant intermolecular force in ammonia (NH3) is hydrogen bonding. Hydrogen bonding occurs between the hydrogen atom of one ammonia molecule and the lone pair of electrons on the nitrogen atom of another ammonia molecule. This results in relatively strong interactions between the molecules.
Sugar has stronger intermolecular forces, such as hydrogen bonding, due to its molecular structure that allows for more interactions between its molecules compared to ammonia. Ammonia, on the other hand, primarily exhibits weaker dipole-dipole interactions.
The strongest intermolecular force between hydrogen chloride molecules is dipole-dipole interactions. Hydrogen chloride is a polar molecule with a permanent dipole moment, so the positive hydrogen end of one molecule is attracted to the negative chlorine end of another molecule, leading to dipole-dipole interactions.
hydrogen bonding
Hydrogen bonding, which is the strongest of the intermolecular forces.
The predominant intermolecular force in methane is London dispersion forces, in ammonia it is hydrogen bonding, in nitrogen trifluoride it is dipole-dipole interactions.
The intermolecular forces in Cl2 are London dispersion forces, which are the weakest type of intermolecular force. This occurs due to temporary fluctuations in electron distribution.
The strongest intermolecular force in NaBr is ionic bonding, which occurs between Na+ cations and Br− anions. Ionic bonds are strong electrostatic attractions between oppositely charged ions.