According to the valence bond theory, Electrons in a molecule occupy atomic orbitals rather than molecular orbitals. The overlapping of atomic orbitals results in the formation of a chemical bond and the electrons are localized in the bond region due to overlapping.
Valence Bond (VB) Theory is a fundamental concept in chemistry that uses the methods of quantum mechanics to explain chemical bonding. Here are the key points:
1. Basic Assumption: VB theory assumes that all bonds are localized bonds formed between two atoms by the donation of an electron from each atom. This, however, is an oversimplification as many atoms bond using delocalized electrons.
2. Focus: It focuses on how the atomic orbitals of the dissociated atoms combine to give individual chemical bonds when a molecule is formed. In contrast, molecular orbital theory has orbitals that cover the whole molecule.
3. Electronic Structure: The theory describes the electronic structure of molecules. It states that electrons fill the atomic orbitals of an atom within a molecule.
4. Covalent Bond: VB theory describes a covalent bond as the overlap of half-filled atomic orbitals (each containing a single electron) that yield a pair of electrons shared between the two bonded atoms.
5. Historical Development: The theory has been developed and refined over time by many scientists, including G.N. Lewis, Charles Rugeley Bury, Kossel, Walter Heitler, Fritz London, and Linus Pauling.
Please note that while VB theory provides a useful model for understanding chemical bonding, it does have its limitations and is not able to accurately describe all types of chemical bonds or molecular structures.
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According to the valence bond theory, Electrons in a molecule occupy atomic orbitals rather than molecular orbitals. The overlapping of atomic orbitals results in the formation of a chemical bond and the electrons are localized in the bond region due to overlapping.
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Valence Bond (VB) Theory is a fundamental concept in chemistry that uses the methods of quantum mechanics to explain chemical bonding. Here are the key points:
1. Basic Assumption: VB theory assumes that all bonds are localized bonds formed between two atoms by the donation of an electron from each atom. This, however, is an oversimplification as many atoms bond using delocalized electrons.
2. Focus: It focuses on how the atomic orbitals of the dissociated atoms combine to give individual chemical bonds when a molecule is formed. In contrast, molecular orbital theory has orbitals that cover the whole molecule.
3. Electronic Structure: The theory describes the electronic structure of molecules. It states that electrons fill the atomic orbitals of an atom within a molecule.
4. Covalent Bond: VB theory describes a covalent bond as the overlap of half-filled atomic orbitals (each containing a single electron) that yield a pair of electrons shared between the two bonded atoms.
5. Historical Development: The theory has been developed and refined over time by many scientists, including G.N. Lewis, Charles Rugeley Bury, Kossel, Walter Heitler, Fritz London, and Linus Pauling.
Please note that while VB theory provides a useful model for understanding chemical bonding, it does have its limitations and is not able to accurately describe all types of chemical bonds or molecular structures.