Hydrogen (H2) is a diatomic molecule consisting of two hydrogen atoms. In its molecular form, H2 does not possess significant intermolecular forces due to its nonpolar nature.
The primary intermolecular force present in H2 is London dispersion forces, which are the weakest type of intermolecular attraction. These forces arise from the temporary fluctuations in electron density that create instantaneous dipoles in the molecules. Even though hydrogen molecules are nonpolar and lack permanent dipoles, the presence of London dispersion forces allows for very weak attractions between H2 molecules.
In summary, H2 primarily exhibits London dispersion forces as its intermolecular force, characterized by their minimal strength and significance in simple molecular interactions.