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Hybridisation Basics, Orbital Picture Video Lecture | Crash Course for IIT JAM Chemistry
FAQs on Hybridisation Basics, Orbital Picture Video Lecture - Crash Course for IIT JAM Chemistry
| 1. What is hybridization in chemistry? |  |
Ans. Hybridization in chemistry refers to the mixing of atomic orbitals to form new hybrid orbitals. This process occurs when atoms bond together to form molecules. Hybrid orbitals have different shapes and energies compared to the atomic orbitals from which they are derived.
| 2. Why is hybridization important in chemistry? | |
Ans. Hybridization is important in chemistry because it helps explain the geometry and bonding properties of molecules. By understanding the hybridization of atoms within a molecule, we can predict the molecular shape, bond angles, and the types of bonds formed. This information is crucial in understanding the reactivity and properties of molecules.
| 3. What are the different types of hybridization? | |
Ans. The different types of hybridization include sp, sp2, sp3, sp3d, sp3d2, and sp3d3. These types of hybridization correspond to the different geometries and bond angles observed in molecules. For example, sp hybridization results in linear geometry, sp2 hybridization results in trigonal planar geometry, and sp3 hybridization results in tetrahedral geometry.
| 4. How does hybridization affect the bonding in a molecule? | |
Ans. Hybridization affects the bonding in a molecule by determining the type and strength of the bonds formed. Different hybrid orbitals have different shapes and orientations, which allow for optimal overlap with other orbitals during bonding. This overlap leads to the formation of sigma bonds, pi bonds, or both, depending on the type of hybridization.
| 5. How does hybridization explain the double bond in molecules like ethene (C2H4)? | |
Ans. In ethene (C2H4), each carbon atom undergoes sp2 hybridization. This means that three atomic orbitals from each carbon atom (2p orbitals and 1s orbital) combine to form three sp2 hybrid orbitals. These hybrid orbitals arrange themselves in a trigonal planar geometry, with one remaining p orbital perpendicular to the plane. The unhybridized p orbitals from each carbon atom then overlap sideways to form a pi bond, resulting in a double bond between the carbon atoms.
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Dec 22, 2024 Last updated |
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