Concept:Diatomic hydrogen (\( \text{H}_2 \)) is a perfectly non-polar molecule with a completely symmetrical electron cloud.
Formula:Not applicable.
Solution:- Within an \( \text{H}_2 \) molecule, the two hydrogen atoms are held by a non-polar covalent bond.
- However, the question asks for the force among separate \( \text{H}_2 \) molecules in a solid crystal lattice.
- Because \( \text{H}_2 \) is strictly non-polar and lacks any highly electronegative atom (N, O, F), it cannot form dipole-dipole interactions or hydrogen bonds.
- The only possible forces between these non-polar molecules are instantaneous induced-dipole attractions, collectively known as London dispersion forces, which fall under the umbrella category of Van der Waals forces.
Why other options are incorrect:Covalent bonds exist
inside the molecule, not
between them. Hydrogen bonding is strictly impossible because there is no F, O, or N present.
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