Assignment Use Online Sources To Review Theories

Assignmentuse Online Sources To Learnreview The Theories Of Covalen

Assignment: Use online sources to learn/review the theories of covalent bonding. Remember to cite your sources in APA style Objectives: Describe the valence bond (VB) approach to chemical bonding and the molecular orbital (MO) theory Demonstrate hybridization of atomic orbitals for VB & MO Correlate the molecular shape to the hybrid atomic orbitals of some central atoms. Combine the concepts of hybrid orbitals, valence bond theory, VSEPR, resonance structures, and octet rule to describe the shapes and structures of some common molecules. . Background: Compare and contrast the VB theory and the MO theory by applying at least two chemical compounds; the central themes of both theories; hybridization, Hund’s rule, Lewis Structures, the VSEPR theory. Resonance, molecular shapes and polarity. 350 words only

Paper For Above instruction

Covalent bonding remains a fundamental concept in chemistry, explaining how atoms share electrons to achieve stable electronic configurations. Two primary theories elucidate this bonding: the Valence Bond (VB) theory and Molecular Orbital (MO) theory, each offering unique insights into molecular structures and behaviors.

The Valence Bond theory emphasizes the overlap of atomic orbitals, where electrons are localized between specific pairs of atoms. It posits that chemical bonds are formed when atomic orbitals hybridize, combining to create new, degenerate orbitals that enable effective overlap. Hybridization, such as sp³ in methane, explains the tetrahedral shape by combining one s orbital and three p orbitals. VB theory also incorporates concepts like Lewis structures and the octet rule, which predict molecular shapes and bonding patterns based on electron pairing and repulsion, as explained through the VSEPR model. For instance, in water, the central oxygen atom’s sp³ hybridization results in a bent shape due to lone pairs.

Conversely, the Molecular Orbital theory describes bonding by combining atomic orbitals across the entire molecule to form molecular orbitals that extend over multiple atoms. Electrons occupy these orbitals, which can be bonding or antibonding, providing a delocalized view. MO theory accounts for phenomena like resonance and molecular stability more comprehensively than VB. For example, benzene’s delocalized π electrons are better explained through MO theory’s π molecular orbitals, reinforcing its aromatic stability.

Both theories underscore important concepts like hybridization and Hund’s rule. Hund’s rule, stating electrons fill degenerate orbitals singly before pairing, influences the electronic configuration within hybrid or molecular orbitals, affecting molecular shapes and magnetic properties. Additionally, resonance structures in molecules like ozone or benzene depict electron delocalization, aligning with MO theory perspectives, which justify their stability and planar shapes.

In conclusion, while VB theory provides an intuitive, localized view of bonding aligned with classical concepts of hybridization and electron pairs, MO theory offers a comprehensive, delocalized understanding useful for explaining aromaticity and resonance. Together, these theories elucidate the varied and complex nature of covalent molecules, their shapes, and properties, enhancing our understanding of chemical bonding’s fundamental principles.

References

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