Would a substance that does not form hydrogen bonds have a high or low surface tension? What about vapor pressure, specific heat,heat of vaporization or boiling point?
It requires extra energy to break hydrogen bonds so a substance that does not form H bonding can evaporate easier (higher vapor pressure, lower boiling point etc) all other things being equal. Remember that other things besides H bonding affect some of those values.
A substance that does not form hydrogen bonds would have a low surface tension compared to a substance that does form hydrogen bonds. Surface tension is the cohesive force that exists between the liquid molecules at the surface, and hydrogen bonding contributes significantly to this force. Without hydrogen bonding, the molecules in the liquid do not have strong attractions to each other, resulting in lower surface tension.
Regarding vapor pressure, specific heat, heat of vaporization, and boiling point, these properties are influenced by various factors, not just hydrogen bonding. However, the absence of hydrogen bonding can contribute to changes in these properties.
A substance that does not form hydrogen bonds will generally have a higher vapor pressure. This is because, in the absence of strong intermolecular forces like hydrogen bonding, the molecules can more easily escape from the liquid phase and enter the gas phase. Increased vapor pressure means that the substance evaporates more readily.
Specific heat is the amount of heat energy required to raise the temperature of a substance by a certain amount. It is not directly affected by the presence or absence of hydrogen bonds. However, the absence of hydrogen bonding may indirectly influence specific heat if the specific heat of the substance is affected by other intermolecular forces or molecular structure.
The heat of vaporization is the amount of heat energy required to convert a substance from its liquid phase to its gas phase at its boiling point. A substance that does not form hydrogen bonds generally has a lower heat of vaporization. This is because hydrogen bonding contributes to the stability of the liquid phase, and breaking these bonds requires extra energy. Without strong hydrogen bonding, the intermolecular forces holding the molecules in the liquid phase are weaker, requiring less energy to vaporize the substance.
Finally, the boiling point is the temperature at which a substance changes from its liquid phase to its gas phase. The absence of hydrogen bonding can result in a lower boiling point. This is because hydrogen bonding provides extra stability to the liquid phase, and without it, the molecules can more easily escape into the gas phase, leading to a lower boiling point.
It's important to note that while hydrogen bonding is one of the major factors influencing these properties, other factors such as molecular size, shape, and intermolecular forces other than hydrogen bonding can also contribute to variations in these properties.