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Video: Molecular Orbital Theory Video Lecture | Physical Chemistry for NEET

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FAQs on Video: Molecular Orbital Theory Video Lecture - Physical Chemistry for NEET

1. What is molecular orbital theory and how does it explain the bonding between atoms?
Ans. Molecular orbital theory is a model used in chemistry to explain the bonding between atoms in a molecule. It describes how atomic orbitals combine to form molecular orbitals, which can be bonding or antibonding in nature. In this theory, electrons are distributed in these molecular orbitals based on their energy levels, resulting in the formation of covalent bonds between atoms.
2. What are the key differences between molecular orbital theory and valence bond theory?
Ans. Molecular orbital theory and valence bond theory are two different models used to explain chemical bonding. The key differences lie in their approaches. Molecular orbital theory considers the entire molecule as a whole, with electrons distributed in molecular orbitals formed by the combination of atomic orbitals. Valence bond theory, on the other hand, focuses on the overlapping of atomic orbitals to form covalent bonds between atoms. While molecular orbital theory provides a more comprehensive description, valence bond theory emphasizes the localized nature of bonding.
3. How does molecular orbital theory explain the stability of molecules?
Ans. Molecular orbital theory explains the stability of molecules by analyzing the energy levels and occupancy of molecular orbitals. A stable molecule is formed when the total number of bonding electrons exceeds the number of antibonding electrons in the molecular orbitals. This leads to a net stabilization of the molecule, as the bonding electrons contribute to a lower overall energy. Additionally, the distribution of electrons in the molecular orbitals determines the strength of the bonds and overall stability of the molecule.
4. Can molecular orbital theory be applied to all types of chemical bonds?
Ans. Molecular orbital theory is primarily applicable to covalent bonds, where electrons are shared between atoms. It provides a comprehensive understanding of the bonding in molecules formed through covalent interactions. However, it is less applicable to ionic bonds, where electrons are transferred between atoms, or metallic bonds, which involve delocalized electrons. For these types of bonds, other theories such as the crystal field theory or band theory are more suitable.
5. How does molecular orbital theory explain the concept of bond order?
Ans. Bond order is a concept used in molecular orbital theory to indicate the strength and stability of a covalent bond. It is calculated by subtracting the number of antibonding electrons from the number of bonding electrons and dividing the result by 2. A higher bond order indicates a stronger bond, as it signifies a greater number of bonding electrons compared to antibonding electrons. This relationship is a direct consequence of the molecular orbital theory, where the occupancy of molecular orbitals determines the bonding characteristics between atoms.
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