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Valence Bond Theory Video Lecture - Class 11

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1. What is Valence Bond Theory?
Ans. Valence Bond Theory is a chemical bonding theory that describes the formation of covalent bonds between atoms. According to this theory, a covalent bond is formed by the overlap of atomic orbitals, where each orbital contains a single electron with opposite spins.
2. How does Valence Bond Theory explain the concept of hybridization?
Ans. Valence Bond Theory explains the concept of hybridization by proposing that atomic orbitals can combine to form hybrid orbitals. These hybrid orbitals have different shapes and energies compared to the original atomic orbitals, allowing for the formation of stronger and more stable covalent bonds.
3. What is the role of overlapping orbitals in Valence Bond Theory?
Ans. Overlapping orbitals play a crucial role in Valence Bond Theory. When the atomic orbitals of two atoms overlap, the electron density between the two nuclei increases, resulting in a covalent bond. The type and extent of orbital overlap determine the strength and nature of the bond formed.
4. Can Valence Bond Theory explain molecular shapes and bond angles?
Ans. Yes, Valence Bond Theory can explain molecular shapes and bond angles through the concept of hybrid orbitals. The hybridization of atomic orbitals determines the geometry of a molecule, and the angles between the hybrid orbitals dictate the bond angles in the molecule's structure.
5. How does Valence Bond Theory differ from Molecular Orbital Theory?
Ans. Valence Bond Theory and Molecular Orbital Theory are both theories used to explain chemical bonding. Valence Bond Theory focuses on the overlap of atomic orbitals to form bonds, while Molecular Orbital Theory considers the combination of atomic orbitals to form molecular orbitals. Valence Bond Theory emphasizes the localization of electrons in specific bonds, whereas Molecular Orbital Theory describes the delocalization of electrons throughout the entire molecule.
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