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Energy can be in many forms: below I have written how a liquid evaporates, which tells you about the average kinetic energy of particles. It relates to inTERmolecular bonding, although I'm not sure if you are also looking at inTRAmolecular bonding too.

Firstly, you should know that as a phase change is being undertaken (as a substance changes from solid, liquid or gas into something else), the temperature remains constant. Now you know that, I'll tell you why.

The average kinetic energy of a substance (the energy it has to move around ie. the speed of the particles) is directly proportional to the absolute temperature, in kelvin. ie. If the temperature is 0K (zero kelvin, or -273.15ºC), there is NO movement of any particles. If the temperature is 100K (or -173.15ºC) there is SOME movement of particles. If the temperature is 373.15K (or 100ºC), there is GREATER movement of particles. ie. The higher the temperature, the higher the speed of the particles, and the higher the speed of the particles, the higher the temperature of the substance.

There are intermolecular forces (ie. Van der Waal's forces, dipole-dipole forces and hydrogen bonding forces) that attract multiple molecules together. To overcome these forces, ie. to break free of these forces so that a particle can leave the liquid, that particle must have a lot of energy, enough to overcome the particular intermolecular forces (some are stronger than others - the three above are in order of weakest --> strongest respectively).

Some particles in a liquid have more energy than others. ie. some move faster than others. These particles are more likely to 'break free' of the forces and evaporate. When one of these higher-energy particles leaves the liquid, the average kinetic energy of the liquid decreases. Hence because average kinetic energy is directly proportional to temperature, the overall temperature decreases a little.

Sorry if its a bit of a confusing explanation! You really should know how one thing works to know how another works, so I tried using a little detail in it. ! :)

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10y ago

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