<p>um...how do you estimate and compare dipole moments between molecules again? I think the answer to the Cl2 and HCl question had to do with dipole moments and LDFs.</p>
<p>curious also. I got destroyed on this question.</p>
<p>Yes, it does. I talked about polarity and the electronegativity of the molecule. The more the electrons in a molecule the biggest chance that at any given point in time, there will be dipole moments. Bigger chance of dipoles = stronger attractive forces. Therefore bigger molecules tend to be stronger than smaller ones.</p>
<p>Yeah, Cl2 is larger, and therefore more polarizable, which makes the bonds stronger despite the fact that HCl has a net dipole moment and therefore stronger intermolecular forces. I got lucky on this question.</p>
<p>Strictly speaking, the question had little to do with net dipole moments, but if one felt like adding relevant but unnecessary information, I could see how one could mention them.</p>