Which of the following best explains the fact that H2S boils at -60 Celsius while H2O boils at 100 Celsius at normal atmospheric pressure?
Both H2O and H2S exhibit London dispersion forces, but the dispersion forces are stronger in H2O
H2O has a larger net dipole moment than H2S.
H2O exhibits hydrogen bonding interactions while H2S does not.
H2O has London dispersion forces while H2S does not.
H2O has a smaller mass than H2S