Valence Bond Theory || 4 Marks in 10 Minutes For NEET Exam

Competition Wallah・2 minutes read

Physics Valhalla offers quick lessons and question-solving sessions on covalent bond formation, emphasizing electron sharing and bond energy release. The text details the importance of proper orbital alignment and phase overlap in creating strong sigma and pi bonds for increased stability.

Insights

  • When atoms form covalent bonds, the sharing of electrons from their balance cells leads to the creation of bond energy, releasing energy as the atoms come closer. The relationship between potential energy and internuclear distance, illustrated through a graph, showcases the crucial bond length necessary for maintaining the bond.
  • The formation of molecular orbitals through phase overlap, whether positive or negative, determines bond formation. Positive-positive and negative-negative overlaps facilitate bond creation, while positive-negative overlaps hinder it. Sigma bonds, resulting from molecular axis overlap, are stronger than pi bonds due to better lobe merging, emphasizing the significance of proper alignment, as seen in scenarios involving dx a and py orbitals at a 39-degree angle, preventing bond formation.

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Summary

00:00

"Covalent Bond Theories: Physics Valhalla Explained"

  • Physics Valhalla is a platform where concepts are taught and previous year questions are solved within 10 minutes.
  • The topic discussed is Balance Bond Theories, focusing on the formation of covalent bonds when atoms join.
  • The process involves the sharing of electrons from the balance cells of two atoms.
  • An example with hydrogen atoms illustrates how nuclei attract electrons, leading to the formation of a bond.
  • Energy is released when two hydrogens come closer, forming a bond known as bond energy.
  • A graph of potential energy and internuclear distance shows the relationship between energy and distance in bond formation.
  • The internuclear distance between two nuclei is referred to as bond length, crucial for maintaining the bond.
  • Molecular orbitals are formed when atoms combine, increasing electron density between nuclei.
  • Phase overlap, whether positive or negative, determines bond formation between orbitals.
  • Positive overlap occurs when like phases overlap, while negative overlap hinders bond formation.

13:20

Orbital Overlaps Determine Bond Formation Strength

  • Overlapping of orbitals is crucial for bond formation; positive-positive and negative-negative overlaps lead to bond formation, while positive-negative overlaps result in no bond formation.
  • Sigma bond formation occurs when orbitals overlap along the molecular axis, resulting in the merging of lobes from different orbitals.
  • Pi bond formation involves perpendicular overlapping of orbitals along the molecular axis, leading to side-wise overlapping and the creation of pi bonds.
  • Sigma bonds are stronger than pi bonds due to better overlapping, resulting in increased electron density between nuclei and enhanced stability.
  • In a scenario where dx a and py orbitals are involved, their overlapping along the molecular axis at 39 degrees prevents bond formation, highlighting the importance of proper alignment for bond creation.
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