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Ch.9 - Molecular Geometry and Bonding Theories
All textbooksBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblem 55a,b
Chapter 9, Problem 55a,b

(a) Draw a picture showing how two p orbitals on two different atoms can be combined to make a σ bond. (b) Sketch a π bond that is constructed from p orbitals.

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1
Step 1: Understand the concept of orbital overlap. In chemistry, a σ bond is formed when two atomic orbitals overlap along the axis connecting the two nuclei. This is typically a head-on overlap.
Step 2: Visualize the p orbitals. A p orbital has a dumbbell shape with two lobes. When two p orbitals from different atoms approach each other, they can overlap to form a σ bond if they align along the internuclear axis.
Step 3: Draw the σ bond formation. Sketch two p orbitals from different atoms with their lobes pointing towards each other along the axis connecting the two nuclei. The overlap region between the lobes represents the σ bond.
Step 4: Understand the π bond formation. A π bond is formed when two p orbitals overlap side-by-side, above and below the internuclear axis, rather than head-on.
Step 5: Sketch the π bond. Draw two p orbitals from different atoms parallel to each other, with their lobes overlapping side-by-side. The overlap region above and below the internuclear axis represents the π bond.

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Key Concepts

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

Orbital Hybridization

Orbital hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that can accommodate bonding. In the case of p orbitals, two p orbitals from different atoms can overlap to form a sigma (σ) bond, which is characterized by head-on overlap, allowing for strong bonding between the atoms.
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Sigma (σ) and Pi (π) Bonds

Sigma (σ) bonds are formed by the end-to-end overlap of orbitals, which can include s and p orbitals, resulting in a bond that allows for free rotation around the bond axis. In contrast, pi (π) bonds are formed by the side-to-side overlap of p orbitals, which occurs above and below the bond axis, restricting rotation and contributing to the double or triple bond character in molecules.
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Molecular Orbital Theory

Molecular orbital theory describes how atomic orbitals combine to form molecular orbitals that can be occupied by electrons. This theory helps explain the bonding and anti-bonding interactions between orbitals, providing a framework for understanding the stability and properties of molecules formed by the combination of p orbitals, particularly in the context of σ and π bonds.
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Related Practice
Textbook Question
(c) Write the formulas for the analogousspecies of the elements of period 3;
Textbook Question

(a) Which geometry and central atom hybridization would you expect in the series BH4-, CH4, NH4+?

Textbook Question

(b) What would you expect for the magnitude and direction of the bond dipoles in this series?

Textbook Question

(c) Which is generally stronger, a s bond or a p bond? Explain.

Textbook Question

(d) Can two s orbitals combine to form a p bond? Explain.