This high degree of symmetry is the decisive factor in answering the initial question. If dipole-dipole forces were significant, the boiling point would be substantially higher.
Why Methane's Bond Dipoles Cancel Out Completely
7°F) at standard pressure, existing as a gas under ambient conditions. The individual bond dipoles are vectors that point from hydrogen toward carbon.
Since methane is a nonpolar molecule due to its symmetric charge distribution, it does not possess a permanent dipole moment required to engage in dipole-dipole interactions with other methane molecules. The Actual Forces Present in Methane Because methane lacks a permanent dipole, dipole-dipole forces are not present in its physical interactions.
How Symmetry Causes Methane's Bond Dipoles to Cancel
Methane, lacking this permanent polarity, relies solely on the much weaker London forces. Water has a bent geometry, which prevents the bond dipoles from canceling out, resulting in a strong net dipole moment.
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