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Chapter 9: Problem 56

(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?

Short Answer

Expert verified
(a) In an sp hybridized atom, there are 2 unhybridized p orbitals and it can form 2 π bonds. (b) It is easier to twist around a single σ bond than around a double bond (σ + π) due to the rigid nature of the π bond.

Step by step solution

01

(a) Determine the number of unhybridized p orbitals

sp hybridization occurs when one s-orbital combines with one p-orbital to form two hybrid orbitals. Since p orbitals are three in number (px, py, and pz), the remaining unhybridized p orbitals will be 2 (px and py if we assume the pz gets hybridized).
02

Determine the number of π bonds an atom with sp hybridization can form

An unhybridized p orbital can form one π bond. As there are two unhybridized p orbitals in an sp hybridized atom (from the previous step), the atom can form two π bonds.
03

(b) Comparing the ease of twisting around a single σ bond and a double bond (σ + π)

A single σ bond allows free rotation around the bond axis without affecting the bond length. In contrast, a π bond does not allow free rotation due to the parallel arrangement of electron cloud above and below the plane, holding the atoms together more rigidly. Thus, rotation around a double bond (σ+π) would require energy to break the π bond, making it harder to twist compared to a single σ bond. So, it would be easier to twist (rotate) around a single σ bond than around a double bond (σ + π).

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Most popular questions from this chapter

Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle.

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