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Chapter 9: Problem 9

In the hybrid orbital model, compare and contrast \(\sigma\) bonds with \(\pi\) bonds. What orbitals form the \(\sigma\) bonds and what orbitals form the \(\pi\) bonds? Assume the \(z\) -axis is the internuclear axis.

Short Answer

Expert verified
In the hybrid orbital model, \(\sigma\) bonds are formed by the axial overlap of s and p orbitals along the internuclear axis, resulting in strong, stable, and polar bonds due to significant orbital overlap and electron density between the nuclei. On the other hand, \(\pi\) bonds are formed by the lateral overlap of parallel p orbitals above and below the internuclear axis, leading to weaker, less polar bonds with less significant orbital overlap.

Step by step solution

01

Understanding sigma (\(\sigma\)) bonds and their formation

A \(\sigma\) bond is formed when two orbitals, one from each atom, overlap end-to-end along the internuclear axis (the line connecting the two nuclei). This overlap is called axial overlap. The resulting bond is strong and stable because of the significant overlap of orbitals along the internuclear axis. In general, s and p orbitals can form \(\sigma\) bonds. For example, an s-s, s-p, or p-p overlap could lead to the formation of a \(\sigma\) bond.
02

Understanding pi (\(\pi\)) bonds and their formation

A \(\pi\) bond is formed when two parallel p orbitals, one from each atom, overlap side-to-side above and below the internuclear axis. This overlap is called lateral overlap. The resulting bond is weaker than a \(\sigma\) bond because the overlap between the orbitals is not as significant (less electron density between the nuclei). In general, only p orbitals can form \(\pi\) bonds, such as a p-p overlap.
03

Comparing and contrasting sigma (\(\sigma\)) and pi (\(\pi\)) bonds

There are several ways in which \(\sigma\) and \(\pi\) bonds can be compared and contrasted: 1. Formation: While \(\sigma\) bonds are formed by the axial overlap of orbitals, \(\pi\) bonds are formed by the lateral overlap of parallel p orbitals. 2. Strength: \(\sigma\) bonds are generally stronger than \(\pi\) bonds, due to the greater orbital overlap and the electron density situated between the nuclei. 3. Orbitals involved: \(\sigma\) bonds can be formed by the overlap of s and p orbitals, whereas \(\pi\) bonds are only formed by the overlap of p orbitals. 4. Polarity: \(\sigma\) bonds are usually more polar than \(\pi\) bonds, as they allow for more charge distribution between the atoms involved. #Conclusion# In summary, \(\sigma\) bonds are stronger, more stable, and polar bonds formed by the axial overlap of s and p orbitals along the internuclear axis. On the other hand, \(\pi\) bonds are weaker, less polar bonds formed by the lateral overlap of parallel p orbitals above and below the internuclear axis.

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Most popular questions from this chapter

Complete the following resonance structures for \(\mathrm{POCl}_{3}\). (A) (B) a. Would you predict the same molecular structure from each resonance structure? b. What is the hybridization of \(\mathrm{P}\) in each structure? c. What orbitals can the \(\mathrm{P}\) atom use to form the \(\pi\) bond in structure \(\mathrm{B}\) ? d. Which resonance structure would be favored on the basis of formal charges?

One of the first drugs to be approved for use in treatment of acquired immune deficiency syndrome (AIDS) was azidothymidine (AZT). Complete the Lewis structure for AZT. a. How many carbon atoms are \(s p^{3}\) hybridized? b. How many carbon atoms are \(s p^{2}\) hybridized? c. Which atom is \(s p\) hybridized? d. How many \(\sigma\) bonds are in the molecule? e. How many \(\pi\) bonds are in the molecule? f. What is the \(\mathrm{N}=\mathrm{N}=\mathrm{N}\) bond angle in the azide \(\left(-\mathrm{N}_{3}\right)\) group? g. What is the \(\mathrm{H}-\mathrm{O}-\mathrm{C}\) bond angle in the side group attached to the five-membered ring? h. What is the hybridization of the oxygen atom in the \(-\mathrm{CH}_{2} \mathrm{OH}\) group?

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Complete the Lewis structures of the following molecules. Predict the molecular structure, polarity, bond angles, and hybrid orbitals used by the atoms marked by asterisks for each molecule. a. \(\mathrm{BH}_{3}\) b. \(\mathrm{N}_{2} \mathrm{~F}_{2}\) c. \(\mathrm{C}_{4} \mathrm{H}_{6}\)

For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur. a. \(\mathrm{SO}_{2}\) b. \(\mathrm{SO}_{3}\) c. d. e. \(\mathrm{SO}_{3}^{2-}\) i. \(\mathrm{SF}_{6}\) f. \(\mathrm{SO}_{4}^{2-}\) j. \(\mathrm{F}_{3} \mathrm{~S}-\mathrm{SF}\) g. \(\mathrm{SF}_{2}\) \(\mathbf{k} . \mathrm{SF}_{5}{ }^{+}\) h. \(\mathrm{SF}_{4}\)
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