Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
10th Edition
ISBN: 9781305957510
Author: ZUMDAHL, Steven S.; Zumdahl, Susan A.; DeCoste, Donald J.
Publisher: Cengage Learning
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Textbook Question
Chapter 9, Problem 2ALQ
Explain the difference between the σ and π MOs for homonuclear diatomic molecules. How are bonding and antibonding orbitals different? Why are there two π MOs and one σ MO? Why are the π MOs degenerate?
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Chapter 9 Solutions
Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
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- Why is the concept of hybridization required in valence bond theory?arrow_forwardThe molecules N2 and CO are isoelectronic but their properties are quite different. Although as a first approximation we often use the same MO diagram for both, suggest how the MOs in N2 and CO might be different.arrow_forwardWhich of the period 2 homonuclear diatomic molecules are predicted to be paramagnetic?arrow_forward
- Identify the hybrid orbitals used by antimony in SbCl5 and in SbCl6, the ion formed from the reaction of SbCl5 and Cl. Explain your choices.arrow_forwardConsider a heteronuclear diatomic molecule, AB, where A and B are period 2 elements. Using the following pieces of information, provide details on the molecular orbital diagram of AB: Clue 1: The MO diagram of AB does not contain non- bonding electrons. Clue 2: The s and p orbital energies of both atoms are quite close to one another that interactions between different orbital types occur. Clue 3: AB" is more stable than AB, but AB2 is less stable than AB". Clue 4: The potential energies of the atomic orbitals of A are higher than the potential energies of the atomic orbitals of B. Table 1. Atomic orbital energies of period 2 elements. Atom Orbital energy Orbital energy (2s) (2p) Li -5.45 Ве -9.30 B -14.0 -8.30 C -19.5 -10.7 -25.5 -13.1 -32.3 -15.9 F -46.4 -18.7 Ne -48.5 -21.5arrow_forwardWould you expect the Be2 molecule to be stable in the gas phase? What is the total bond order, and how many net σ and π bonds are there?arrow_forward
- Study the following sketch of a molecular orbital (MO) in a homonuclear diatomic molecule. This MO was formed by combining one 2p atomic orbital from atom. The dark dots in this sketch are the nuclei. Now use the sketch to complete the table below. Write the symbol for this MO. Is this a bonding or antibonding MO? What is the energy of this MO, compared to the energy of a 2p orbital on one of the separate 0 Obonding antibonding O higher Olower the same not enough information to decide D 8 70 % 9arrow_forwardWrite drawbacks of Valence Bond Theory .arrow_forwardWhen is a resonance hybrid needed to adequately depict the bonding in a molecule? Using NO₂ as an example, explain how aresonance hybrid is consistent with the actual bond length, bond strength, and bond order.arrow_forward
- When considering molecular orbital diagrams of homonuclear diatomic molecules, explain why atomic orbital energies are the same. How will this differ for heteronuclear diatomic molecules?arrow_forwardUse molecular orbital theory to explain why the Be2 molecule does not exist. Determine it's bond order and whether it is paramagnetic or diamagnetic.arrow_forward*71. The MO of the ground state of a heteronuclear diatomic molecule AB is alr mol = CAp + Cx«" If a bonding electron spends 90% of its time in an orbital A on atom A and 10% of its time in ç" on atom B, what are the values of C, and C? (Neglect the overlap of the two orbitals.)arrow_forward
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