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Boiling point increases as a result of a higher intermolecular bond. For example water, which has hydrogen bonding, has stronger bonds than ethanol, which is nonpolar. This is shown by water's higher boiling point.
Professor Lavelle uses boiling points to indicate which dipole interactions are stronger because the stronger the interactions between molecules, the more energy/heat required to separate them from each other, which raises the boiling point of the molecule.
Boiling point is when a liquid goes to the gas phase, and this requires a release of energy, and this comes from the breaking of these intermolecular bonds. But, stronger bonds mean that they are harder to break. In this way, boiling point could be a useful tool for telling us how strong the IMFs are.
The general rule is that, the stronger the intermolecular forces, the harder it is to break them. Thus boiling point is a measure of the strength of forces between atoms in a molecule. The higher the boiling point, the stronger the forces.
When a bond is stronger, it needs more energy to be broken. There is more energy in higher temperature. So when a bond is really strong, it needs more energy to be broken (and go to different state) i.e it has a higher boiling point/melting point. Similarly when a bond is weak, it needs little energy to be broken so the temperature does not need to be that high (low melting/boiling pt)
Natalie Benitez 1C wrote:How can we determine between elements which will have a higher boiling point?
Based on the type of intermolecular forces (so london dispersion and or hydrogen bonding) you can tell which will have higher boiling points. The more attracted molecules are to each other, the higher the boiling point will be.
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