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Chapter 9: Problem 53

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
To determine the hybridization for each pair of hybrid orbitals, compare their characteristic angles with the angles associated with sp, sp2, and sp3 hybridizations. Specifically, look for angles close to 180° for sp hybridization, 120° for sp2 hybridization, and 109.5° for sp3 hybridization. Determine the most suitable hybridization for each pair based on these comparisons.

Step by step solution

01

Pair 1:

To find the hybridization, compare the given angle with the characteristic angles of sp, sp2, and sp3 hybridizations: - sp hybridization: linear geometry with a characteristic angle of 180° - sp2 hybridization: trigonal planar geometry with a characteristic angle of 120° - sp3 hybridization: tetrahedral geometry with a characteristic angle of 109.5° Now, compare the angle of the given pair with these characteristic angles, and determine which hybridization is the most suitable.
02

Pair 2:

Repeat the same process as in Pair 1. Compare the angle of the given pair with the characteristic angles of sp, sp2, and sp3 hybridizations. Determine the most suitable hybridization based on this comparison.
03

Pair 3:

Repeat the same process as in Pair 1 and Pair 2. Compare the angle of the given pair with the characteristic angles of sp, sp2, and sp3 hybridizations. Determine the most suitable hybridization based on this comparison.

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Most popular questions from this chapter

(a) Draw Lewis structures for chloromethane $\left(\mathrm{CH}_{3} \mathrm{Cl}\right),\( chloroethene \)\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}\right)\(, and chloroethyne \)\left(\mathrm{C}_{2} \mathrm{HCl}\right) .(\mathbf{b})$ What is the hybridization of the carbon atoms in each molecule? (c) Predict which molecules, if any, are planar. (d) How many \(\sigma\) and \(\pi\) bonds are there in each molecule?

Place the following molecules and ions in order from smallest to largest bond order: $\mathrm{N}_{2}{ }_{2}^{2+}, \mathrm{He}_{2}{ }^{+}, \mathrm{Cl}_{2} \mathrm{H}_{2}^{-}, \mathrm{O}_{2}{ }^{2-}$.

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

Name the proper three-dimensional molecular shapes for each of the following molecules or ions, showing lone pairs as needed: $(\mathbf{a}) \mathrm{ClO}_{2}^{-}(\mathbf{b}) \mathrm{SO}_{4}^{2-}(\mathbf{c}) \mathrm{NF}_{3}(\mathbf{d}) \mathrm{CCl}_{2} \mathrm{Br}_{2}(\mathbf{e}) \mathrm{SF}_{4}^{2+}$

Ethyl propanoate, $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOCH}_{2} \mathrm{CH}_{3},$ gives a fruity pineapple-like smell. (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds. (b) How many \(\sigma\) and how many \(\pi\) bonds are in the molecule? (c) Which CO bond is shortest in the molecule? (d) What is the hybridization of atomic orbitals around the carbon atom associated with that short bond? (e) What are the approximate bond angles around each carbon atom in the molecule?
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