it is polar. therefore, dipole-dipole and dispersion forces (always present)
dipole dipole forces
dipole-dipole
These are London dispersion forces.
hydrogen
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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.
Dipole forces and London forces are present as intermolecular forces in these molecules.
These are intermolecular forces.
The intermolecular forces in acetone are weaker.
H2CO; H2CO is polar, whereas CH3CH3 is nonpolar. H2CO has dipole forces in addition to LD forces. CH3CH3 only has LD forces.
CH3NH2 has the higher boiling point as it has a hydrogen bond between the molecule which is a stronger intermolecular attractive force, whereas CH3CH3 only has covalent bonds which are weaker intermolecular attractive forces.
These are polar forces, intermolecular forces of attraction between molecules.
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.