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Superior is a difficult term. The latest versions valence bond theory and molecular orbital theories give similar answers. The simple old versions work from different premises- valence bond assumes localised pair bonds molecular orbital theory is better ate predicting spectroscopic properties. VSEPR is different again and focuses on the geometry around a central atom- and as such is better than both the simple versions of the other theories.
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What two characteristics of liquid oxygen contradict predictions from the valence bond theory but are explained by the molecular orbital theory?
Liquid oxygen exhibits paramagnetism and a relatively low boiling point, characteristics that contradict predictions from the valence bond theory. Valence bond theory suggests that all electrons in O2 should be paired, leading to diamagnetism; however, molecular orbital theory accounts for the presence of unpaired electrons in the antibonding π* orbitals, resulting in paramagnetism. Additionally, the molecular orbital theory explains the lower boiling point of liquid oxygen compared to other diatomic molecules by considering the weaker intermolecular forces due to its electronic configuration.
What is another name for the molecular orbital theory of bonding in metals?
Another name for the molecular orbital theory of bonding in metals is the band theory. Band theory describes how atomic orbitals combine to form energy bands, which explains the electrical conductivity and other properties of metals. It highlights the overlap of atomic orbitals in a solid, leading to the formation of conduction and valence bands.
How do fluorine atom form negative ions?
it depends on the molecular orbital theory
What are the limitations of valence bond theory?
Valence bond theory has limitations as it provides a limited view of molecular bonding, especially when applied to complex molecules. It does not easily explain the molecular geometry and properties of molecules accurately as it assumes fixed bond angles and shapes. Additionally, it does not account for molecular orbitals and delocalized bonding in a comprehensive manner.
Why Molecular bond Theory is better than Valence bond theory?
Molecular orbital theory is more recent than Valence bond theory. Both theories have their adherents and recently VB theory has had a renaissance. They both have their strengths. Chemists use both and mix/match. Some very familiar concepts used every day by chemists spring originally from VB theory, electronegativity, hybridisation of atomic orbitals. MO theory has its advocates, an early triumph was the prediction of the paramagnetism of O2 whereas valence bond theory predicted O2 to be diamagnetic. One criticism of VB theory is that it starts from a description of bonds as localised pairs of electrons, whereas in MO all bonds are potentially delocalised.
What are the key differences between valence bond theory and molecular orbital theory in explaining chemical bonding?
Valence bond theory focuses on the overlap of atomic orbitals to form bonds between atoms, emphasizing the localized nature of bonding. Molecular orbital theory considers the entire molecule as a whole, with electrons delocalized over the entire molecule, leading to the formation of molecular orbitals.
What theory provides information concerning both molecular shape and molecular bonding?
The VSEPR (Valence Shell Electron Pair Repulsion) theory provides information about both molecular shape and molecular bonding. It helps predict the geometric shapes of molecules based on the arrangement of electron pairs around the central atom and takes into account the repulsion between electron pairs to determine the overall molecular shape.
What year was the Valence Bond Theory invented?
Gilbert Lewis followed by Linus Pauling who is credited with the quantum mechanical approach, called valence bond theory (distinguishing it from the more recent molecular orbital theory), which is based on Lewis's electron pair bonding theory now taught as Lewis "dot" diagrams.
What two characteristics of liquid oxygen contradict predictions from the valence bond theory but are explained by the molecular orbital theory?
Liquid oxygen exhibits paramagnetism and a relatively low boiling point, characteristics that contradict predictions from the valence bond theory. Valence bond theory suggests that all electrons in O2 should be paired, leading to diamagnetism; however, molecular orbital theory accounts for the presence of unpaired electrons in the antibonding π* orbitals, resulting in paramagnetism. Additionally, the molecular orbital theory explains the lower boiling point of liquid oxygen compared to other diatomic molecules by considering the weaker intermolecular forces due to its electronic configuration.
What is the role of a node in the molecular orbital theory of chemistry?
In molecular orbital theory, a node is a point in a molecular orbital where the probability of finding an electron is zero. Nodes help determine the shape and energy of the molecular orbital, influencing the chemical properties of the molecule.
What is another name for the molecular orbital theory of bonding in metals?
Another name for the molecular orbital theory of bonding in metals is the band theory. Band theory describes how atomic orbitals combine to form energy bands, which explains the electrical conductivity and other properties of metals. It highlights the overlap of atomic orbitals in a solid, leading to the formation of conduction and valence bands.
Can orbital hybridization theory can describe both the shape and bonding of the molecules?
Orbital hybridization provides information about both molecular bonding and molecular shape.
What is the difference between the homo and lumo energy levels in molecular orbital theory?
In molecular orbital theory, the HOMO (highest occupied molecular orbital) is the highest energy level that contains electrons, while the LUMO (lowest unoccupied molecular orbital) is the lowest energy level that does not contain electrons. The difference between the HOMO and LUMO energy levels determines the reactivity and stability of a molecule.
How do fluorine atom form negative ions?
it depends on the molecular orbital theory
What are the limitations of valence bond theory?
Valence bond theory has limitations as it provides a limited view of molecular bonding, especially when applied to complex molecules. It does not easily explain the molecular geometry and properties of molecules accurately as it assumes fixed bond angles and shapes. Additionally, it does not account for molecular orbitals and delocalized bonding in a comprehensive manner.
Why band theory based on molecular orbital theory?
Band theory is rooted in molecular orbital theory because it explains the electronic structure of solids by considering the overlap of atomic orbitals from adjacent atoms. When atoms come together to form a solid, their discrete molecular orbitals combine to create bands of energy levels, resulting in the formation of valence and conduction bands. This framework helps to characterize electrical conductivity, insulators, and semiconductors, as the distribution of electrons in these bands determines their ability to conduct electricity. Thus, band theory provides a comprehensive understanding of the behavior of electrons in crystalline solids.
What areThe limitations of different bonding models?
Lewis structures: Do not account for molecular geometry and resonance. VSEPR theory: Only predicts molecular shape and does not explain bond strength. Valence bond theory: Simplifies bonding by considering overlapping atomic orbitals, but can be limited in explaining complex molecules. Molecular orbital theory: Provides a more accurate description of bonding but can be complex and computationally expensive for large molecules.
