10 2. Draw the four n-molecular orbitals for the molecule butadiene, drawn below.Label the four orbitals as bonding, non-bonding or antibonding. Which of thefour orbitals are occupied? Which is the LUMO and which is the HOMO?sib laidio mlunal4 Pi electronsby88-Dgilnoo slengoggu or o ed bos 2olunolom od om baod1915b owi ni 29luoslom pasbuloni otolduob orb juodsohib owiow nisiqxoHSG CH38888OCH-CH?CCICHCCHCH?

molecular orbital of 1,3- butadiene is drawn first and then 4 electrons are filled according to…

Answered: Draw the fourR-molecular orbitals for…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Covalent Bonding: Orbitals

Section: Chapter Questions

Problem 41E: Consider the following molecular orbitals formed from the combination of two hydrogen 1s orbitals:...

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The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) CN (b) CO (c) BeB (d) BC+ Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds form from hybrid orbitals: sigma or pi? Explain.
In terms of the molecular orbital model, which species in each of the following two pairs will roost likely be the one to gain an electron? Explain. a. CN or NO b. O22+ or N22+
Two variations of the octahedral geometry (see Table 4-1) are illustrated below. Which of the compounds/ions Br3, ClF3, XeF4, SF4, PF5, ClF5, and SF6 have these molecular structures?
In the hybrid orbital model, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.
Which atomic orbitals overlap to form the bonds in ClF?
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) LiBe+ (b) CO+ (c) CN (d) OF Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Which of the following molecules or ions are para-magnetic? What is the highest occupied molecular orbital (HOMO) in each one? Assume the molecular orbital diagram in Figure 9.16 applies to all of them. (a) NO (b) OF (c) O22 (d) Ne2+
Consider the following molecular orbitals formed from the combination of two hydrogen 1s orbitals: a. Which is the bonding molecular orbital and which is the antibonding molecular orbital? Explain how you can tell by looking at their shapes. b. Which of the two molecular orbitals is lower in energy? Why is this true?
Compare Figs. 4-47 and 4-49. Why are they different? Because B2 is known to be paramagnetic, the 2p and 2p molecular orbitals must be switched from the first prediction. What is the rationale for this? Why might one expect the 2p to be lower in energy than the 2p? Why cant we use diatomic oxygen to help us decide whether the 2p, or 2p, is lower in energy?

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Draw the fourR-molecular orbitals for the molecule butadiene, drawn below. Label the four orbitals as bonding, non-bonding or antibonding. Which of the four orbitals are occupied? Which is the LUMO and which is the HOMO? sib lelidio mluosiom od warO