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Chapter 9: Problem 57

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.

Short Answer

Expert verified
Compare the characteristic angles of each pair of hybrid orbitals to the known hybridization angles: 180° for sp, 120° for sp2, and 109.5° for sp3. For each pair, if the given angle matches one of these angles, that is the type of hybridization for that pair.

Step by step solution

01

Recall the different types of hybridization and their angles

There are 3 main types of hybridizations which are: 1. sp Hybridization: Linear geometry with a characteristic angle of 180° 2. sp2 Hybridization: Trigonal planar geometry with a characteristic angle of 120° 3. sp3 Hybridization: Tetrahedral geometry with a characteristic angle of 109.5° Now, let's analyze each pair of hybrid orbitals to determine the type of hybridization.
02

Compare the characteristic angle of the first pair to the known hybridization angles

Determine the type of hybridization, if any, for the first pair of the hybrid orbitals with the given characteristic angle. Compare the angle to the known hybridization angles 180°, 120°, and 109.5°. If the given angle matches any of these angles, then that's the type of hybridization for the first pair.
03

Compare the characteristic angle of the second pair to the known hybridization angles

Determine the type of hybridization, if any, for the second pair of the hybrid orbitals with the given characteristic angle. Compare the angle to the known hybridization angles 180°, 120°, and 109.5°. If the given angle matches any of these angles, then that's the type of hybridization for the second pair.
04

Compare the characteristic angle of the third pair to the known hybridization angles

Determine the type of hybridization, if any, for the third pair of the hybrid orbitals with the given characteristic angle. Compare the angle to the known hybridization angles 180°, 120°, and 109.5°. If the given angle matches any of these angles, then that's the type of hybridization for the third pair.

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Most popular questions from this chapter

(a) What is the probability of finding an electron on the internuclear axis if the electron occupies a \(\pi\) molecular orbital? (b) For a homonuclear diatomic molecule, what similarities and differences are there between the \(\pi_{2 p}\) MO made from the \(2 p_{x}\) atomic orbitals and the \(\pi_{2 p}\) MO made from the \(2 p_{y}\) atomic orbitals? (c) How do the \(\pi_{2 p}^{*}\) MOs formed from the \(2 p_{x}\) and \(2 p_{y}\) atomic orbitals differ from the \(\pi_{2 p}\) MOs in terms of energies and electron distributions?

Many compounds of the transition-metal elements contain direct bonds between metal atoms. We will assume that the \(z\) -axis is defined as the metal-metal bond axis. (a) Which of the \(3 d\) orbitals (Figure 6.23\()\) can be used to make a \(\sigma\) bond between metal atoms? (b) Sketch the \(\sigma_{3 d}\) bonding and \(\sigma_{3 d}^{*}\) antibonding MOs. (c) With reference to the "Closer Look" box on the phases of orbitals, explain why a node is generated in the \(\sigma_{3 d}^{\star}\) MO. (d) Sketch the energy-level diagram for the \(\mathrm{Sc}_{2}\) molecule, assuming that only the \(3 d\) orbital from part (a) is important. (e) What is the bond order in \(\mathrm{Sc}_{2}\) ?

(a) What is the difference between a localized \(\pi\) bond and a delocalized one? (b) How can you determine whether a molecule or ion will exhibit delocalized \(\pi\) bonding? (c) Is the \(\pi\) bond in \(\mathrm{NO}_{2}^{-}\) localized or delocalized?

(a) Draw a picture showing how two \(p\) orbitals on two different atoms can be combined to make a sigma bond. (b) Sketch a \(\pi\) bond that is constructed from \(p\) orbitals. (c) Which is generally stronger, a \(\sigma\) bond or a \(\pi\) bond? Explain. (d) Can two \(s\) orbitals combine to form a \(\pi\) bond? Explain.

(a) What are the relationships among bond order, bond length, and bond energy? (b) According to molecular orbital theory, would either \(\mathrm{Be}_{2}\) or \(\mathrm{Be}_{2}{ }^{+}\) be expected to exist? Explain.
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