NEET > Chemistry Class 11 > Short Tricks: Dipole Moment
Short Tricks: Dipole Moment Video Lecture - Chemistry Class 11 - NEET
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FAQs on Short Tricks: Dipole Moment Video Lecture - Chemistry Class 11 - NEET
| 1. What is the concept of dipole moment? |  |
Ans. Dipole moment is a measure of the polarity of a chemical bond or a molecule. It represents the separation of positive and negative charges in a molecule, and is defined as the product of the charge and the distance between the charges.
| 2. How is dipole moment calculated for a molecule? | |
Ans. The dipole moment of a molecule can be calculated by multiplying the magnitude of the charge on each atom by the distance between the charges. The dipole moment is a vector quantity and its direction is from the positive to the negative charge.
| 3. What factors affect the dipole moment of a molecule? | |
Ans. Several factors contribute to the dipole moment of a molecule. These include the difference in electronegativity between atoms, the shape of the molecule, and the presence of lone pairs of electrons. A larger difference in electronegativity or a more polar bond will result in a higher dipole moment.
| 4. How does the dipole moment affect the physical properties of a molecule? | |
Ans. The dipole moment of a molecule has a significant impact on its physical properties. It affects the molecule's polarity, boiling point, melting point, and solubility in polar solvents. Molecules with higher dipole moments tend to have stronger intermolecular forces and higher boiling points.
| 5. Can molecules with zero dipole moment have polar bonds? | |
Ans. Yes, molecules can have polar bonds but still have a zero dipole moment if the polar bonds are arranged symmetrically. This occurs when the polar bonds cancel out each other's dipole moments due to the molecular geometry. An example of such a molecule is carbon dioxide (CO2).
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