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In my chemisrty homework, it is requesting me to describe what happens, in terms of particles what happens when bromine, in liquid form reaches its boiling point. You've got be quite detailed. Thanks!!
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Answers (2)
Actually, boiling occurs at the temperature where the vapor pressure of the liquid is EQUAL to the atmospheric pressure. Bromine molecules are held together by London dispersion forces. At the boiling point the added energy is going into breaking those molecular attractions which allow molecules of Br2 to transfer from the liquid to the vapor phase. Since the boiling bromine is not in equilibrium with its vapor, since the gaseous Br2 molecules are free to move into the "entire" atmosphere, the system shifts from the liquid state to the vapor state at the boiling point, and the bromine boils away.
When the vapor pressure of the bromine exceeds the atmospheric pressure on the surface of the liquid the liq will boil. The heat is needed to break the intermolecular attractions between the molecules of the bromine to escape. You can get the liquid to boil at lower temperatures by decreasing the pressure on the surface of the liquid.