What is the Difference Between Polar and Dipolar Molecules?
🆚 Go to Comparative Table 🆚The difference between polar and dipolar molecules lies in the distribution of electrical charges within the molecule and the presence of polar bonds. Here are the key differences:
- Polar Molecules: These molecules have a charge distribution that is not symmetric, resulting from having polar bonds and a molecular geometry that is not symmetric. A polar bond occurs when there is a difference in electronegativity between the two atoms in the bond, causing an unequal charge distribution between the atoms. The sum of the dipole moments of these polar bonds is not equal to zero.
- Dipolar Molecules: These molecules have two poles, meaning they have two opposite ends with opposite electrical charges. Dipole moments can occur between two ions in an ionic bond or between atoms in a covalent bond. In a dipolar molecule, the vector sum of all the individual bond polarities results in an overall molecular polarity.
In summary, polar molecules have a net dipole moment due to the presence of polar bonds and an asymmetric molecular geometry, while dipolar molecules have two poles with opposite electrical charges. The terms polar and dipolar are often used interchangeably, but they describe different aspects of molecular polarity.
Comparative Table: Polar vs Dipolar Molecules
The main difference between polar and dipolar molecules lies in the distribution of electric charge within the molecule. Here is a comparison table highlighting the differences:
| Property | Polar Molecules | Dipolar Molecules |
|---|---|---|
| Definition | Polar molecules have an uneven distribution of electric charge, resulting in a dipole. Part of the molecule has a partial positive charge, and part has a partial negative charge. | Dipolar molecules are a special case of polar molecules, where the bond dipoles do not cancel each other out, resulting in a net dipole moment. |
| Shape | Asymmetric shape, with lone electron pairs or central atom bonded to other atoms with different electronegativity values. | Linear shape, with bond dipoles that do not cancel each other out. |
| Examples | - Water (H2O) - Ammonia (NH3) |
- Carbon dioxide (CO2) - Hydrogen cyanide (HCN) |
| Intermolecular Forces | Stronger intermolecular forces due to hydrogen bonding and dipole-dipole interactions. | Weaker intermolecular forces due to London dispersion forces. |
| Solubility | Soluble in polar solvents. | Insoluble in polar solvents, soluble in nonpolar solvents. |
| Melting and Boiling Points | Higher melting and boiling points due to stronger intermolecular forces. | Lower melting and boiling points due to weaker intermolecular forces. |
In summary, polar molecules have an uneven distribution of electric charge, leading to a dipole, while dipolar molecules are a specific type of polar molecules with bond dipoles that do not cancel each other out. The shape, intermolecular forces, solubility, and melting and boiling points are also different between these two types of molecules.
- Polar Bonds vs Polar Molecules
- Polarizability vs Dipole Moment
- Bond Dipole vs Molecular Dipole
- Polar vs Nonpolar
- Covalent vs Polar Covalent
- Polar vs Nonpolar Covalent Bonds
- Electric Dipole vs Magnetic Dipole
- Ion Dipole vs Dipole Dipole Forces
- Polar vs Nonpolar Solvents
- Dipole Dipole Interactions vs Hydrogen Bonding
- Electronegativity vs Polarity
- Zwitterion vs Dipole
- Polar vs Nonpolar Amino Acids
- Bond Moment vs Dipole Moment
- Induced Dipole vs Permanent Dipole
- Dipole-Dipole vs London Dispersion Forces
- Dipole Dipole vs Dispersion
- Molecules vs Compounds
- Atom vs Molecule