What is the Difference Between Dipole Dipole Interactions and Hydrogen Bonding?
🆚 Go to Comparative Table 🆚Dipole-dipole interactions and hydrogen bonding are both intermolecular forces that occur between molecules, but they differ in their specific characteristics and strength.
Dipole-dipole interactions:
- These interactions occur between polar molecules, which have a permanent dipole due to the difference in electronegativity between atoms.
- The partially negatively charged region of one molecule is attracted to the partially positively charged region of another molecule.
- Dipole-dipole interactions are weaker than hydrogen bonding.
Hydrogen bonding:
- Hydrogen bonding is a specific type of dipole-dipole interaction that occurs between a hydrogen atom bonded to a highly electronegative atom (N, O, or F) and another molecule containing a lone pair of electrons on a highly electronegative atom.
- Hydrogen bonding is stronger than regular dipole-dipole interactions due to the greater electronegativity difference between the hydrogen atom and the highly electronegative atoms (N, O, or F).
- Hydrogen bonds are temporary and last only fractions of a second.
In summary, hydrogen bonding is a specific type of dipole-dipole interaction that occurs between hydrogen atoms bonded to highly electronegative atoms (N, O, or F) and other molecules containing lone pairs of electrons on highly electronegative atoms. Hydrogen bonding is stronger than regular dipole-dipole interactions due to the greater electronegativity difference between the hydrogen atom and the highly electronegative atoms.
Comparative Table: Dipole Dipole Interactions vs Hydrogen Bonding
Dipole-dipole interactions and hydrogen bonding are both types of intermolecular forces, which are the forces of attraction between molecules. However, there are differences between the two. Here is a table comparing the two:
| Feature | Dipole-Dipole Interactions | Hydrogen Bonding |
|---|---|---|
| Definition | Intermolecular forces that occur between polar molecules. | A special type of strong dipole-dipole bonding that occurs between O, N, F, and H atoms. |
| Occurrence | Occur between any polar molecules. | Occur specifically between a hydrogen atom bonded to O, N, or F and another O, N, or F atom. |
| Bond Strength | Weaker than hydrogen bonding. | Stronger than other dipole-dipole interactions due to the high electronegativity of O, N, and F atoms. |
| Examples | Interactions between polar molecules such as HCl and water. | Interactions in water molecules, DNA base pairs, and alcohols. |
In summary, dipole-dipole interactions are intermolecular forces that occur between polar molecules, while hydrogen bonding is a specific type of strong dipole-dipole interaction that occurs between O, N, F, and H atoms. Hydrogen bonding is stronger than other dipole-dipole interactions due to the high electronegativity of O, N, and F atoms.
- Hydrogen Bond vs Ionic Bond
- Ion Dipole vs Dipole Dipole Forces
- Bond Dipole vs Molecular Dipole
- Hydrogen Bond vs Covalent Bond
- Intermolecular vs Intramolecular Hydrogen Bonding
- Bond Moment vs Dipole Moment
- Dipole-Dipole vs London Dispersion Forces
- Van der Waals vs Hydrogen Bonds
- Electric Dipole vs Magnetic Dipole
- Polar vs Dipolar Molecules
- Polarizability vs Dipole Moment
- Zwitterion vs Dipole
- Dipole Dipole vs Dispersion
- Van der Waals vs Hydrophobic Interactions
- Ionic vs Electrostatic Interactions
- Induced Dipole vs Permanent Dipole
- Salt Bridge vs Hydrogen Bond
- Polar Bonds vs Polar Molecules
- Hydrogen Atom vs Hydrogen Ion