ILoveMaths07
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"The solid-liquid phase boundary in the phase diagram of most substances has a positive slope; the greater the pressure on a given substance, the closer together the molecules of the substance are brought to each other, which increases the effect of the substance's intermolecular forces. Thus, the substance requires a higher temperature for its molecules to have enough energy to break out the fixed pattern of the solid phase and enter the liquid phase. A similar concept applies to liquid-gas phase changes. Water, because of its particular properties, is one of the several exceptions to the rule."
What peculiar properties are they talking about? The hydrogen bond? But how does the presence of hydrogen bonds lower the temperature needed for water molecules to have enough energy to break out the fixed pattern of the solid state, and enter the liquid state?
What peculiar properties are they talking about? The hydrogen bond? But how does the presence of hydrogen bonds lower the temperature needed for water molecules to have enough energy to break out the fixed pattern of the solid state, and enter the liquid state?