Arrange the following intermolecular attractions in order of increasing strengtgh:
Dipole interactions, dispersion forces, and hydrogen bonds.
http://www.science.uwaterloo.ca/~cchieh/cact/c123/intermol.html
dispersion forces, hyrdogen bonds then dipole interactions? is this right
Typical hydrogen bonds are about 15-20 kJ/mol and dipole-dipole bonds are about 4 kJ/mol; therefore, I would rank dipole-dipole in the middle. Hydrogen bonds actually are a form of dipole-dipole bonds but they usually are discussed separately and are exclusively called hydrogen bonds when H is attracted to N, F, or O.
To answer the question and arrange the intermolecular attractions in order of increasing strength, we can consider the following:
1. Dispersion forces: These are also known as London forces or van der Waals forces. They are the weakest intermolecular attractions and arise due to temporary fluctuations in electron distribution, creating temporary dipoles in molecules. Dispersion forces act between all molecules, regardless of polarity.
2. Dipole interactions: Dipole-dipole interactions occur between polar molecules. In these interactions, the positive end of one molecule attracts the negative end of another molecule. Dipole interactions are stronger than dispersion forces because they involve permanent dipoles rather than temporary fluctuations.
3. Hydrogen bonds: Hydrogen bonds are a specific type of dipole-dipole interaction that occurs when a hydrogen atom is bonded directly to highly electronegative elements like nitrogen (N), oxygen (O), or fluorine (F). Hydrogen bonds are the strongest among the three intermolecular attractions mentioned.
So, the correct order of increasing strength would be: dispersion forces < dipole interactions < hydrogen bonds.
For more information and to validate this information, you can refer to the provided link: http://www.science.uwaterloo.ca/~cchieh/cact/c123/intermol.html