Final answer:
Molecular oxygen (O₂) experiences only London dispersion forces as its intermolecular force since it is a nonpolar molecule without hydrogen atoms bonded to highly electronegative elements.
Step-by-step explanation:
The types of intermolecular forces present in O₂ can be ascertained by examining the nature of the molecule. Oxygen (₂) is a diatomic, nonpolar molecule without any permanent dipole moment, and it is not capable of forming hydrogen bonds since it does not have hydrogen attached to a highly electronegative atom like fluorine, oxygen, or nitrogen. The primary intermolecular force present in O₂ is the London dispersion force. This force arises from the motion of electrons, which can create temporary dipoles as the electron density fluctuates. Larger molecules tend to have stronger London dispersion forces due to greater electron cloud which can be more easily perturbed. Although O₂ has a moderate size, it will still have these forces present. No dipole-dipole or hydrogen bonding interactions are seen with molecular oxygen.