Answer:
London dispersion forces are the only type of intermolecular forces that nonpolar molecules exhibit.
The molecules in SO2 (g) exhibit dipole-dipole intermolecular interactions.
CH3CH2CH3 has stronger London dispersion forces than does CH4.
Explanation:
London forces result from temporary shifts or distortion in the electron cloud of non-polar molecules. London forces occur in all substances; whether polar or non-polar. However, it is the only kind of intermolecular force in non-polar molecules and noble gases.
Polarity in a molecule stems from difference in electronegativity between the atoms in the molecule. SO2 is a polar molecule due to the magnitude of electronegativity difference between sulphur and oxygen. Hence SO2 exhibit dipole-dipole intermolecular interactions since it is a polar molecule.
The magnitude of London dispersion forces depends on the molar mass and surface area of molecules. CH3CH2CH3 has a higher molar mass and larger surface area than CH4 hence CH3CH2CH3 has stronger London dispersion forces than does CH4.
The following statements which are true include
London forces are the only type of intermolecular force found in non polar
compounds and they are responsible for their attractive interactions.
The molecules in SO2 (g) exhibit dipole-dipole intermolecular interactions as
a result of it being polar.
CH3CH2CH3 has stronger London dispersion forces than does CH4
because it is more non-polar and it is the characteristic attraction found in
non-polar compounds.
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