NEET > Chemistry Class 11 > Polarity of Bonds
Polarity of Bonds Video Lecture - Chemistry Class 11 - NEET
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FAQs on Polarity of Bonds Video Lecture - Chemistry Class 11 - NEET
| 1. What is the definition of polarity in chemical bonds? |  |
Ans. Polarity in chemical bonds refers to the unequal sharing of electrons between two atoms. It occurs when one atom has a higher electronegativity than the other, resulting in a partial positive charge on one atom and a partial negative charge on the other.
| 2. How is the polarity of a bond determined? | |
Ans. The polarity of a bond is determined by the difference in electronegativity between the two atoms involved in the bond. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. The greater the difference in electronegativity, the more polar the bond.
| 3. What are the different types of bond polarities? | |
Ans. There are three types of bond polarities: polar covalent, nonpolar covalent, and ionic. In a polar covalent bond, there is an unequal sharing of electrons between the atoms, resulting in a partial positive and partial negative charge. In a nonpolar covalent bond, there is an equal sharing of electrons between the atoms, resulting in no charge separation. In an ionic bond, one atom completely transfers electrons to another, resulting in the formation of ions with opposite charges.
| 4. How does the polarity of a bond affect the physical properties of a substance? | |
Ans. The polarity of a bond greatly influences the physical properties of a substance. Polar substances have higher boiling points, melting points, and solubilities in polar solvents due to the presence of stronger intermolecular forces of attraction. Nonpolar substances, on the other hand, have lower boiling points, melting points, and solubilities in polar solvents.
| 5. Can a molecule with polar bonds be nonpolar overall? | |
Ans. Yes, a molecule with polar bonds can be nonpolar overall. This occurs when the polar bonds in the molecule are arranged symmetrically, canceling out the overall dipole moment. For example, carbon dioxide (CO2) has polar bonds due to the difference in electronegativity between carbon and oxygen. However, the molecule as a whole is nonpolar because the dipoles of the two polar bonds point in opposite directions, resulting in a net dipole moment of zero.
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195 videos|337 docs|190 tests
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Timeline
| 01:33 | Charge Asymmetry & Geometric Asymmetry |
| 01:49 | Difference in Electronegatives |
| 03:49 | Dipole Moment |
| 04:12 | Charge Separation of a Molecule |
| 04:41 | Like Dissolves Like |
| 05:10 | Water is Awesome |
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