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A molecule can do dipole-dipole bonding if it is polar. It can do hydrogen bonding if it is polar and if it has an OH- or NH- bond. H-bonding is basically a type of dipole-dipole bonding, except with OH and NH bonds. All molecules have London dispersion forces, which are momentary attractive charges formed between molecules when electrons are on one side of a molecule and protons are on the other.
The post above pretty much sums it all up so here's a link if you want extra information: https://chem.libretexts.org/Bookshelves ... rown_et_al.)/11%3A_Liquids_and_Intermolecular_Forces/11.2%3A_Intermolecular_Forces
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