Dipole-dipole interactions, and London dispersion interactions
just dispersion forces, but it can have an induced dipole if its by other electronegative molecule or ion
Dipole-dipole
Dispersion only
dipole-dipole attraction
london dispersion forces
H2CO; H2CO is polar, whereas CH3CH3 is nonpolar. H2CO has dipole forces in addition to LD forces. CH3CH3 only has LD forces.
These are polar forces, intermolecular forces of attraction between molecules.
Yes; all compounds possess London dispersion forces between their molecules, because all compounds contain electrons. However, in the case of H2CO, this will not be the strongest intermolecular force. The strongest will be dipole-dipole interaction, because H2CO is a polar molecule.
Dipole forces and London forces are present as intermolecular forces in these molecules.
These are intermolecular forces.
H2CO; H2CO is polar, whereas CH3CH3 is nonpolar. H2CO has dipole forces in addition to LD forces. CH3CH3 only has LD forces.
These are polar forces, intermolecular forces of attraction between molecules.
Yes; all compounds possess London dispersion forces between their molecules, because all compounds contain electrons. However, in the case of H2CO, this will not be the strongest intermolecular force. The strongest will be dipole-dipole interaction, because H2CO is a polar molecule.
Dipole forces and London forces are present as intermolecular forces in these molecules.
These are intermolecular forces.
Intramolecular forces are not intermolecular forces !
The intermolecular forces in acetone are weaker.
hydrogen bonding
Intermolecular forces in C3CH2CH2NH2London disperiondipole-dipolehydrogen-bonding forces
The weakest of the four forces is gravity by a huge margin
The intermolecular forces are hydrogen bonding.
When there is more thermal energy, then there are less intermolecular forces.