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Boiling points are dependent on the strength of force. The boiling point of a molecule is higher if the bonds are stronger because it takes more energy to break the bonds. So a molecule with shorter bonds will tend to have a higher boiling point.
If a question asks which molecule has the highest boiling point, find out what type of bonding is within each molecule. The strongest are ionic bonds (ion-ion), then ion-dipoles, then hydrogen bonds, then dipole-dipoles, then LDF. The stronger the bond, the higher the boiling point.
Nick Lewis 3D wrote:Essentially, does this mean that boiling points have a direct correlation to electronegativity? I would think that if an atom is more electronegative then there is a stronger bond and thus a higher boiling point.
I would say it is more about the difference in electronegativities between atoms in a compound that the electronegativity of each atom itself. More electronegatively different atoms in a molecule makes the molecule more and more ionic (to the extent that it actually is an ionic compound), which makes it have a higher boiling point.
It ultimately boils down (haha get it) to the strength of the bonds that are present in the compound. If bond strengths are greater, it takes more energy to weaken them thus requiring greater heat to provide that energy.
Boiling points increase as the strength of the intermolecular forces increases. For example, a molecule with Hydrogen bonds will likely have a higher boiling point than a molecule with only induced dipole forces because the Hydrogen bonds require more energy to break. Higher temperatures have more energy.
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