What is the Difference Between Bond Moment and Dipole Moment?
🆚 Go to Comparative Table 🆚The key difference between bond moment and dipole moment lies in their definitions and the scope of their application. Here are the main distinctions:
- Bond Moment: Also known as bond dipole moment, it represents the polarity of a chemical bond within a molecule. It occurs when there is a separation of positive and negative charges in a chemical bond, typically due to differences in electronegativity between the bonded atoms.
- Dipole Moment: This is a measure of any electrical separation, including charge separations in molecules and lone pairs of electrons, if any. The dipole moment of a molecule is the vectorial addition of individual bond moments and moments due to lone pairs (if any).
In summary:
- Bond moment refers to the polarity of a specific chemical bond within a molecule, while dipole moment encompasses the overall electrical separation in the molecule, including contributions from multiple bond moments and lone pairs of electrons.
- Bond moment is more focused on the intramolecular charges and their separation within a specific bond, whereas dipole moment considers the overall charge distribution and separation in the entire molecule.
On this pageWhat is the Difference Between Bond Moment and Dipole Moment? Comparative Table: Bond Moment vs Dipole Moment
Comparative Table: Bond Moment vs Dipole Moment
The difference between bond moment and dipole moment can be understood through the following table:
| Property | Bond Moment | Dipole Moment |
|---|---|---|
| Definition | Bond moment refers to the polarity in a covalent chemical bond between two atoms with different electronegativities. | Dipole moment is the separation of electrical charges, which can occur between two ions in an ionic bond or between atoms in a covalent bond. |
| Occurrence | Occurs in covalent bonds with different electronegativities. | Occurs in both ionic and covalent bonds. |
| Cause | Caused by the different electronegativities of the bonded atoms. | Caused by the difference between electronegativity values of different atoms. |
| Mathematical Representation | Not represented as a vector quantity. | Represented as a vector quantity, with both magnitude and direction. |
| Measurement | Harder to measure directly. | Easier to measure, as it can be determined by placing a substance between charged plates. |
In summary, bond moment refers to the polarity in a covalent bond between two atoms with different electronegativities, while dipole moment is the separation of electrical charges in both ionic and covalent bonds. Dipole moment is a vector quantity, with both magnitude and direction, and is easier to measure compared to bond moment.
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