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They don't - quite the opposite!

Boiling point depends on the strength of intermolecular forces and on the molecular weight of the molecule.

One factor contributing to intermolecular forces is an asymmetrical distribution of electric charge - in this case, the dipole charges of adjacent molecules can orient towards each other and allow for increased bonding strength. Conversely, in a symmetrical molecule this cannot occur, so the bonds will be weaker. This means that all other factors being equal, an symmetrical molecule will have weaker intermolecular bonds and thus a lower boiling point.

For example, a symmetric methane molecule (weight ~16) boils at a lower temperature than the less-symmetric ammonia (NH3, weight ~17), which in boils at a lower temperature than the very asymmetric water (H2O, weight ~18) depite the fact that their weights are nearly identical.

Conversely, a very highly symmetric radon gas atom remains a gas at room temperature despite a weight of 222 g/mol.

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