- #1
jaydnul
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I saw a video on youtube saying water molecules were held together by hydrogen bonding, not dipole dipole. Why is that?
Van der WaalsAbdulQat said:But two H atoms or two H2 molecules undergo dipole-dipole dispersive interactions without having permanent dipoles.
Their orientations are correlated, which gives an effective attraction even if the average orientation of each atom is random.Likewise for two orientation-averaged H2O molecules.
Ice is like many frozen hydrogen bonds, and the high melting/boiling point is a result of hydrogen bonds in ice and water. As gas, interactions between atoms are weak as always.Can it be measured in any or all phases of H2O?
A hydrogen bond is a specific type of dipole-dipole interaction that occurs between a hydrogen atom and a highly electronegative atom, such as oxygen or nitrogen. It is a stronger type of dipole-dipole interaction due to the large difference in electronegativity between the two atoms involved.
A hydrogen bond is generally stronger than a regular dipole-dipole interaction. This is because the hydrogen bond involves a highly electronegative atom, resulting in a larger separation of charge and a stronger attraction between the molecules.
Molecules that contain hydrogen bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine, can form hydrogen bonds. Common examples include water, ammonia, and hydrogen fluoride.
Hydrogen bonds between water molecules give it unique properties, such as high surface tension, boiling point, and heat capacity. These bonds also allow water to dissolve many substances, making it an excellent solvent.
No, dipole-dipole interactions only occur between polar molecules. Non-polar molecules have a symmetrical distribution of charge and therefore do not have a dipole moment, making them unable to form dipole-dipole interactions.