What is the Difference Between Bond Dipole and Molecular Dipole?
🆚 Go to Comparative Table 🆚The difference between a bond dipole and a molecular dipole lies in their definitions and the scope of their application. Here are the key differences:
- Bond Dipole: A bond dipole is a measure of the separation of electronic charge between two atoms bonded together. It is determined by the difference in electronegativity between the two atoms. If the electronegativity difference is large, the bond is considered polar, and a bond dipole moment is present. Examples of bond dipoles can be found in molecules containing the most electronegative elements, such as oxygen, nitrogen, and halogens.
- Molecular Dipole: A molecular dipole, or molecular dipole moment, is the net dipole for the entire molecule, which is the vector sum of all the bond dipoles in the molecule. It takes into account not only the individual bond moments but also how these dipoles are arranged in the molecular structure. The overall dipole moment of a molecule determines its molecular polarity.
In summary:
- A bond dipole is a measure of the separation of electron density between two atoms within a molecule.
- A molecular dipole is the net dipole moment for the entire molecule, considering the vector sum of all individual bond dipoles.
On this pageWhat is the Difference Between Bond Dipole and Molecular Dipole? Comparative Table: Bond Dipole vs Molecular Dipole
Comparative Table: Bond Dipole vs Molecular Dipole
The difference between bond dipole and molecular dipole can be summarized in the following table:
| Feature | Bond Dipole | Molecular Dipole |
|---|---|---|
| Definition | A bond dipole is the presence of two opposite charged ends in the same chemical bond, resulting from the unequal sharing of electrons between the bonded atoms. | A molecular dipole is the presence of two opposite charged ends in the same molecule, arising due to the net polarity of the molecule. |
| Dipole Moment | Bond dipole moment is the electric dipole moment that occurs when there is a separation of charge within a bond. | Molecular dipole moment is the net dipole moment for the entire molecule, which is the vector sum of all individual bond dipoles. |
| Polarity | Bond polarity refers to the presence of two opposite charged ends in a particular chemical bond. | Molecular polarity refers to the overall polarity of a molecule, which can be determined by considering the shape of the molecule and the polarity of its individual bonds. |
| Electronegativity | A wide difference in electronegativity between the bonded atoms causes polarity in the bond and results in a bond dipole. | The net polarity or overall polarity of a molecule comes with the effect of the shape of the molecule, sometimes causing a molecule with polar chemical bonds not to have a net polarity due to the shape that balances. |
For example, in a diatomic molecule like HCl, the bond dipole and molecular dipole are the same because there is only one bond between the two atoms. In molecules with multiple bonds, the molecular dipole is the net result of all individual bond dipoles.
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- Hydrogen Bond vs Ionic Bond
- Ionic vs Molecular Solids
- Double Bond vs Single Bond