A concept map for four types of intermolecular forces and a certain type of bond is shown. Which of the following correctly identifies the intermolecular force represented by A and compares its strength relative to the intermolecular force represented by b.

1. A represents London dispersion forces, which are weaker than the force represented by b
2. A represents hydrogen bonding, which is weaker than the force represented by b
3. A represents London dispersion forces, which are stronger than the force represented by b
4. A represents hydrogen bonding, which is stronger than the force represented by b

There are four major classes of interactions between molecules and they are all different manifestations of “opposite charges attract”. The four key intermolecular forces are as follows: Ionic bonds > Hydrogen bonding > Van der Waals dipole-dipole interactions > Van der Waals dispersion forces.

The strongest intermolecular force is hydrogen bonding, which is a particular subset of dipole-dipole interactions that occur when a hydrogen is in close proximity (bound to) a highly electronegative element (namely oxygen, nitrogen, or fluorine). To determine the intermolecular forces of a molecule or chemical, you must first construct the electron dot structure (Lewis structure). Then you determine the polarity of the molecule. Once you have those done determining the types of intermolecular bonds become much more simple.

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