Final answer:
Decahydronaphthalene primarily exhibits London dispersion forces among intermolecular forces, which are influenced by the molecular size and shape.
Step-by-step explanation:
Intermolecular Forces in Decahydronaphthalene
The primary intermolecular force in decahydronaphthalene is London dispersion forces. These are a type of van der Waals force that occurs between all molecules, whether they are polar or nonpolar. London dispersion forces arise due to the momentary imbalances in electron distribution within molecules, creating temporary dipoles that induce corresponding dipoles in adjacent molecules. The strength of these forces depends on the mass and surface area of the molecule. Because decahydronaphthalene is a larger molecule with a significant surface area, it engages in stronger London dispersion forces than smaller molecules, resulting in higher boiling points and other physical properties influenced by intermolecular interactions. As decahydronaphthalene lacks significant electronegativity differences between its atoms, dipole-dipole interactions and hydrogen bonding are not prominent in this compound.
In summary, decahydronaphthalene primarily exhibits London dispersion forces, which are influenced by its molecular size and shape.