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Chapter 9: Problem 78

Consider three molecules: \(\mathrm{A}, \mathrm{B}\), and \(\mathrm{C}\). Molecule A has a hybridization of \(s p^{3}\). Molecule B has two more effective pairs (electron pairs around the central atom) than molecule A. Molecule C consists of two \(\sigma\) bonds and two \(\pi\) bonds. Give the molecular structure, hybridization, bond angles, and an example for each molecule.

Short Answer

Expert verified
Molecule A: Tetrahedral structure, \(sp^3\) hybridization, bond angle of 109.5 degrees. Example: Methane (CH4). Molecule B: Octahedral structure, \(sp^3d^2\) hybridization, bond angle of 90 degrees. Example: Sulfur hexafluoride (SF6). Molecule C: Trigonal planar structure (one double bond and two single bonds), \(sp^2\) hybridization, bond angle of 120 degrees. Example: Ethene (C2H4).

Step by step solution

01

Molecule A: Hybridization \(sp^3\)

Molecular structure: Tetrahedral Hybridization: \(sp^3\) Bond angles: 109.5 degrees Example: Methane (CH4)
02

Molecule B: 2 more effective pairs than A

Since molecule A has a hybridization of \(sp^3\) with 4 effective pairs (electron pairs around the central atom), molecule B will have 6 effective pairs. This implies that molecule B has an octahedral structure. Molecular structure: Octahedral Hybridization: \(sp^3d^2\) Bond angles: 90 degrees Example: Sulfur hexafluoride (SF6)
03

Molecule C: 2 \(\sigma\) bonds and 2 \(\pi\) bonds

Having two \(\sigma\) bonds and two \(\pi\) bonds indicates that the molecule is a double bond. A compound with one double bond typically has a hybridization of \(sp^2\). Molecular structure: Trigonal planar (one double bond and two single bonds) Hybridization: \(sp^2\) Bond angles: 120 degrees Example: Ethene (C2H4)

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Most popular questions from this chapter

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

Cyanamide \(\left(\mathrm{H}_{2} \mathrm{NCN}\right)\), an important industrial chemical, is produced by the following steps: $$ \begin{aligned} \mathrm{CaC}_{2}+\mathrm{N}_{2} & \longrightarrow \mathrm{CaNCN}+\mathrm{C} \\\ \mathrm{CaNCN} & \stackrel{\text { Acid }}{\longrightarrow} \mathrm{H}_{2} \mathrm{NCN} \end{aligned} $$ Cyanamid Calcium cyanamide (CaNCN) is used as a direct-application fertilizer, weed killer, and cotton defoliant. It is also used to make cyanamide, dicyandiamide, and melamine plastics: a. Write Lewis structures for \(\mathrm{NCN}^{2-}, \mathrm{H}_{2} \mathrm{NCN}\), dicyandiamide, and melamine, including resonance structures where appropriate. b. Give the hybridization of the \(\mathrm{C}\) and \(\mathrm{N}\) atoms in each species. c. How many \(\sigma\) bonds and how many \(\pi\) bonds are in each species? d. Is the ring in melamine planar? e. There are three different \(\mathrm{C}-\mathrm{N}\) bond distances in dicyandiamide, \(\mathrm{NCNC}\left(\mathrm{NH}_{2}\right)_{2}\), and the molecule is nonlinear. Of all the resonance structures you drew for this molecule, predict which should be the most important.

The diatomic molecule OH exists in the gas phase. The bond length and bond energy have been measured to be \(97.06 \mathrm{pm}\) and \(424.7 \mathrm{~kJ} / \mathrm{mol}\), respectively. Assume that the OH molecule is analogous to the HF molecule discussed in the chapter and that molecular orbitals result from the overlap of a lower-energy \(p_{z}\) orbital from oxygen with the higher- energy \(1 s\) orbital of hydrogen (the \(\mathrm{O}-\mathrm{H}\) bond lies along the \(z\) -axis). a. Which of the two molecular orbitals will have the greater hydrogen \(1 s\) character? b. Can the \(2 p_{x}\) orbital of oxygen form molecular orbitals with the \(1 s\) orbital of hydrogen? Explain. c. Knowing that only the \(2 p\) orbitals of oxygen will interact significantly with the \(1 s\) orbital of hydrogen, complete the molecular orbital energy- level diagram for OH. Place the correct number of electrons in the energy levels. d. Estimate the bond order for OH. e. Predict whether the bond order of \(\mathrm{OH}^{+}\) will be greater than, less than, or the same as that of \(\mathrm{OH}\). Explain.

Complete the following resonance structures for \(\mathrm{POCl}_{3}\). 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 struc- ture \(\mathrm{B}\) ? d. Which resonance structure would be favored on the basis of formal charges?

Many important compounds in the chemical industry are derivatives of ethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\). Two of them are acrylonitrile and methyl methacrylate. Complete the Lewis structures, showing all lone pairs. Give approximate values for bond angles \(a\) through \(f\). Give the hybridization of all carbon atoms. In acrylonitrile, how many of the atoms in the molecule must lie in the same plane? How many \(\sigma\) bonds and how many \(\pi\) bonds are there in methyl methacrylate and acrylonitrile?
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