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Chapter 9: Problem 60

(a) If the valence atomic orbitals of an atom are sp hybridized, how many unhybridized \(p\) orbitals remain in the valence shell? How many \(\pi\) bonds can the atom form? (b) Imagine that you could hold two atoms that are bonded together, twist them, and not change the bond length. Would it be easier to twist (rotate) around a single \(\sigma\) bond or around a double \((\sigma\) plus \(\pi)\) bond, or would they be the same? Explain.

Short Answer

Expert verified
(a) There are two unhybridized p orbitals remaining in the valence shell, and the atom can form two π bonds. (b) It would be easier to twist around a single σ bond than around a double bond (σ plus π). This is because the π bond restricts rotation, which creates a higher energy barrier compared to a single σ bond.

Step by step solution

01

Identify hybrid orbitals and number of valence electrons

In sp hybridization, the s and p orbitals are combined to form two new hybrid orbitals, sp. Since there are three p orbitals in the valence shell (px, py, and pz), one of them is used for hybridization with the s orbital, leaving two p orbitals unhybridized.
02

Determine the number of remaining unhybridized p orbitals

Since one p orbital is used for hybridization, there are two unhybridized p orbitals remaining in the valence shell (lets say, py and pz).
03

Determine the number of π bonds possible

Each unhybridized p orbital can form one π bond. Therefore, the atom can form two π bonds. #Answer_Part_A# (a) There are two unhybridized p orbitals remaining in the valence shell, and the atom can form two π bonds. (b)
04

Understand the nature of σ and π bonds

A σ bond is formed by the head-on overlap of orbitals between two atoms, while a π bond is formed by the sideways overlap of orbitals. Because of this, σ bonds allow free rotation, while π bonds restrict rotation, making it difficult to twist the atoms around the bond without breaking the π bond.
05

Compare ease of rotation around a single σ bond and a double bond (σ plus π)

Since a single bond has only a σ bond, rotation around the bond is relatively easy. However, double bonds have both a σ and a π bond, and rotation around the bond requires breaking the π bond causing a higher energy barrier, making it more difficult and energetically unfavorable to twist around a double bond. #Answer_Part_B# (b) It would be easier to twist around a single σ bond than around a double bond (σ plus π). This is because the π bond restricts rotation, which creates a higher energy barrier compared to a single σ bond.

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