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We start with the symmetric possibilities, H2O, OF2, and OCl2. The bond angles and bond lengths of these three molecules are shown below: Note that the bond lengths increase in a way we can understand easily: H is smaller than F, which is smaller than Cl. But look at the bond angles. We have claimed that the two lone pairs on the O atom (not shown) should push the bonding pairs of electrons down, lowering the bond angle from the perfect tetrahedral angle of 109.47Â°.
Here major intermolecular attractive force is hydrogen bonding. The chemicals that exhibit hydrogen bonding, which is a special type of dipole-dipole interactions, are found when you have an H attached to an N, O or F. These are very strong because of the huge differences in electronegativities of the pair, which gives them super strong attractions. To learn more about intermolecular attractive forces visit here