In comparison to molecules that interact by London dispersion forces only, the meling point of similar sized molecu forming hydrogen bonds would most likely be about the same unpredictable lower higher

## Step 1<br />The problem is asking us to compare the melting points of two types of molecules: those that interact only through London dispersion forces and those that form hydrogen bonds. <br /><br />## Step 2<br />London dispersion forces are the weakest type of intermolecular force. They occur due to temporary fluctuations in electron density in a molecule, which create temporary dipoles that can induce dipoles in neighboring molecules. <br /><br />## Step 3<br />On the other hand, hydrogen bonding is a stronger type of intermolecular force. It occurs when a hydrogen atom is bonded to a highly electronegative atom such as nitrogen, oxygen, or fluorine, and is attracted to another electronegative atom in a different molecule.<br /><br />## Step 4<br />Because hydrogen bonding is stronger than London dispersion forces, it requires more energy to break the bonds between molecules. This means that molecules with hydrogen bonds will have higher melting points than those with only London dispersion forces, because more energy is needed to overcome the stronger intermolecular forces.