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Valence Bond Theory - Coordination Chemistry Video Lecture | Inorganic Chemistry
FAQs on Valence Bond Theory - Coordination Chemistry Video Lecture - Inorganic Chemistry
| 1. What is valence bond theory in coordination chemistry? |  |
Ans. Valence bond theory is a model used in coordination chemistry to explain the bonding between a central metal ion and its surrounding ligands. It states that the metal and ligands overlap their atomic orbitals to form a series of covalent bonds, resulting in a complex with a well-defined geometry.
| 2. How does valence bond theory explain the bonding in coordination complexes? | |
Ans. According to valence bond theory, the central metal ion and ligands in a coordination complex each contribute unpaired electrons from their atomic orbitals to form a set of hybrid orbitals. These hybrid orbitals then overlap with each other to form covalent bonds, resulting in the formation of a stable complex.
| 3. What are the limitations of valence bond theory in coordination chemistry? | |
Ans. Valence bond theory has some limitations in explaining certain aspects of coordination chemistry. It does not provide a clear explanation for the color and magnetic properties of coordination complexes. Additionally, it does not account for the influence of crystal field effects on the electronic structure and properties of complexes.
| 4. How does valence bond theory explain the concept of ligand field splitting? | |
Ans. Valence bond theory explains ligand field splitting by considering the interaction between the ligand's electron pair and the d-orbitals of the central metal ion. The ligand's electron pair repels the electrons in the d-orbitals, causing them to split into two energy levels. This splitting results in the formation of different energy levels for the d-orbitals, known as the ligand field splitting.
| 5. How does valence bond theory explain the concept of hybridization in coordination complexes? | |
Ans. Valence bond theory explains hybridization in coordination complexes by considering the mixing of the atomic orbitals of the central metal ion and the ligands. This mixing results in the formation of a set of hybrid orbitals, which have different shapes and energies compared to the original atomic orbitals. The hybrid orbitals then participate in the formation of covalent bonds between the metal ion and ligands.
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