What is the Difference Between Polarizability and Dipole Moment?
🆚 Go to Comparative Table 🆚Polarizability and dipole moment are two distinct concepts in chemistry related to molecules and their electron clouds. The key differences between them are:
- Definition: Polarizability is the measure of how easily an electron cloud is distorted by an electric field, while dipole moment is the separation of positive and negative charges in a system.
- Nature: Polarizability is the tendency of a compound to form a dipole when exposed to an external electric field, whereas a compound's dipole moment is the permanent separation of charge across a distance.
- Relationship: A molecule with a large polarizability does not necessarily have a large dipole moment. In fact, some highly polarizable molecules do not have a dipole moment at all.
- Mathematical Representation: Polarizability is represented by the Greek letter alpha (α), while dipole moment is represented by the Greek letter mu (μ).
In summary, polarizability is the ease with which an electron cloud can be distorted, indicating a compound's tendency to become polarized when exposed to an electric field. On the other hand, dipole moment is the permanent separation of charge within a compound, indicating the polar nature of the compound itself.
Comparative Table: Polarizability vs Dipole Moment
The key difference between polarizability and dipole moment is that polarizability is the measure of how easily an electron cloud is distorted by an external electric field, while dipole moment is the separation of positive and negative charges in a system. Here is a table summarizing the differences between polarizability and dipole moment:
| Property | Polarizability | Dipole Moment |
|---|---|---|
| Definition | The tendency of matter to acquire an electric dipole moment in proportion to the external electric field. | The separation of electrical charges, which may occur between two ions in an ionic bond or two atoms in a covalent bond. |
| Unit of Measurement | None (it's a tendency) | Debye units (1 Debye equals $3.34 \ C\, m)$). |
| Related to | Electron cloud distortion in response to an external electric field. | Separation of positive and negative charges due to differences in electronegativity. |
| Calculation | Induced dipole moment ($ \mu_{induced} = \alpha \vec{E} $). | Dipole moment of a molecule can be calculated using the equation: $ \vec{\mu} = \sumi qi \, \vec{r}_i $. |
| Examples | Molecules with high polarizability tend to have a dipole moment, but not always. | The larger the difference in electronegativity, the larger the dipole moment. |
In summary, polarizability refers to the tendency of a molecule to become polarized in response to an external electric field, while dipole moment is the permanent separation of charge within a molecule or material.
- Bond Moment vs Dipole Moment
- Polar vs Dipolar Molecules
- Electric Dipole vs Magnetic Dipole
- Bond Dipole vs Molecular Dipole
- Induced Dipole vs Permanent Dipole
- Electronegativity vs Polarity
- Zwitterion vs Dipole
- Ion Dipole vs Dipole Dipole Forces
- Dipole Dipole vs Dispersion
- Dipole Dipole Interactions vs Hydrogen Bonding
- Polar vs Nonpolar
- Polar Bonds vs Polar Molecules
- Covalent vs Polar Covalent
- Concentration Polarization vs Kinetic Polarization
- Dipole-Dipole vs London Dispersion Forces
- Polar vs Nonpolar Covalent Bonds
- Polarizable vs Non Polarizable Electrode
- Electropositive vs Electronegative
- Magnetization vs Demagnetization