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Unit 11 - Intermolecular Forces, Liquids, and Solids, Screenshot 2022-05…
Unit 11 - Intermolecular Forces, Liquids, and Solids
11.1 - A Molecular Comparison of Gases, Liquids, and Solids
The fundamental difference between states of matter is the strength of the intermolecular forces of attraction.
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The state of a substance depends largely on the balance between the kinetic energies of the particles and the interparticle energies of attraction
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11.4 - Phase Changes
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Phase changes: melting/freezing, vaporizing/condensing, subliming/depositing.
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11.5 - Vapor Pressure
At any temperature, some liquid molecules have enough energy to escape the surface and become a gas, called evaporation
As the temperature rises, the fraction of molecules that have enough energy to break free increases.
As more molecules escape the liquid, the pressure they exert increases.
The liquid and vapor reach a state of dynamic equilibrium: liquid molecules evaporate and vapor molecules condense at the same rate.
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Liquids with high vapor pressure evaporate more quickly and in an open container, are termed volatile.
The boiling point of a liquid is the temperature at which its vapor pressure equals atmospheric pressure.
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11.6 - Phase Diagrams
The temperature beyond which a gas cannot be compressed is called its critical temperature. This is the highest temperature that a liquid can exist.
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