The following diagrams illustrate p-p orbital overlap or s-porbital overlap. Which diagram represents a p bond in valencebond theory? (LO 8.3)(a)
(b)
(c)
(d)

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Identify the type of orbital overlap in each diagram.

Recall that a π bond is formed by the side-by-side overlap of p orbitals.

Examine each diagram to determine which one shows side-by-side overlap of p orbitals.

Diagram (a) shows p-p orbital overlap with lobes arranged side-by-side.

Conclude that diagram (a) represents a π bond in valence bond theory.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Orbital Overlap

Orbital overlap refers to the interaction between atomic orbitals when atoms approach each other to form a bond. In valence bond theory, the extent of overlap between orbitals determines the strength and type of bond formed. For example, p-p orbital overlap leads to the formation of pi bonds, while s-p overlap typically results in sigma bonds.

Types of Bonds

In chemistry, bonds can be classified into sigma (σ) and pi (π) bonds based on the type of orbital overlap. Sigma bonds occur when orbitals overlap head-on, allowing for free rotation around the bond axis. In contrast, pi bonds form from the side-to-side overlap of p orbitals, which restricts rotation and contributes to the double or triple bond character in molecules.

Valence Bond Theory

Valence bond theory explains how atoms bond by considering the overlap of their atomic orbitals. It emphasizes the role of electron pairs in bonding and describes how different types of orbital overlaps lead to the formation of specific bond types. This theory is fundamental for understanding molecular geometry and the behavior of electrons in chemical bonds.

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