Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory

Tro - Chemistry: A Molecular Approach 4th Edition

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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory

Problem 66

Chapter 10, Problem 66

Write a hybridization and bonding scheme for each molecule that contains more than one interior atom. Indicate the hybridization about each interior atom. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. c. C₂H₆ (skeletal structure H₃CCH₃)

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Identify the interior atoms in the molecule C2H6. In this case, the interior atoms are the two carbon atoms.

Determine the hybridization of each carbon atom. Since each carbon atom in C2H6 forms four single bonds (three with hydrogen atoms and one with the other carbon atom), the hybridization is sp^3.

Sketch the structure of C2H6, showing the two carbon atoms bonded to each other and each carbon atom bonded to three hydrogen atoms.

Illustrate the overlapping orbitals: each C-H bond is formed by the overlap of an sp^3 hybrid orbital from carbon with the 1s orbital of hydrogen, and the C-C bond is formed by the overlap of sp^3 hybrid orbitals from each carbon.

Label all bonds: the C-H bonds are sigma (σ) bonds formed by sp^3-1s overlap, and the C-C bond is a sigma (σ) bond formed by sp^3-sp^3 overlap.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybridization

Hybridization is the process of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of a molecule. In the case of C2H6 (ethane), the carbon atoms undergo sp3 hybridization, resulting in four equivalent sp3 hybrid orbitals that form sigma bonds with hydrogen atoms and between the carbon atoms.

Bonding and Molecular Geometry

The bonding in molecules is determined by the arrangement of hybrid orbitals and the types of bonds formed. In C2H6, each carbon atom forms four sigma bonds, leading to a tetrahedral geometry around each carbon. This geometry influences the overall shape of the molecule, which is crucial for understanding its reactivity and interactions.

Orbital Overlap

Orbital overlap is a key concept in covalent bonding, where atomic orbitals from different atoms combine to form bonds. In C2H6, the overlap of sp3 hybrid orbitals from carbon with the 1s orbitals of hydrogen atoms creates strong sigma bonds. Visualizing this overlap helps in understanding the molecular structure and bond angles.

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Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. d. I₃^-

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Consider the structure of the amino acid aspartic acid. Indicate the hybridization about each interior atom.

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Textbook Question

Draw an MO energy diagram and predict the bond order of Be₂⁺ and Be₂^- . Do you expect these molecules to exist in the gas phase?

Write a hybridization and bonding scheme for each molecule that contains more than one interior atom. Indicate the hybridization about each interior atom. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. N₂H₂ (skeletal structure HNNH) b. N₂H₄ (skeletal structure H₂NNH₂) c. CH₃NH₂ (skeletal structure H₃CNH₂)

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