Organic Chemistry: Structure and Function
8th Edition
ISBN: 9781319079451
Author: K. Peter C. Vollhardt, Neil E. Schore
Publisher: W. H. Freeman
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Chapter 1.7, Problem 1.15TIY
Interpretation Introduction
Interpretation:Themolecular orbital and energy-splitting diagram for the bonding in
Concept Introduction:Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:
- Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.
- Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.
- Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.
Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.
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44. The molecule H3* has long been speculated to exist. The interest here is that the addition
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a) Draw what you think would be the most stable structure for H3* and show all
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b)
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Chapter 1 Solutions
Organic Chemistry: Structure and Function
Ch. 1.3 - Prob. 1.1ECh. 1.3 - Prob. 1.2ECh. 1.3 - Prob. 1.3ECh. 1.3 - Prob. 1.4ECh. 1.3 - Prob. 1.5ECh. 1.4 - Prob. 1.6ECh. 1.4 - Prob. 1.8TIYCh. 1.5 - Prob. 1.9ECh. 1.5 - Prob. 1.11TIYCh. 1.6 - Prob. 1.12E
Ch. 1.6 - Prob. 1.13ECh. 1.7 - Prob. 1.15TIYCh. 1.8 - Prob. 1.16ECh. 1.8 - Prob. 1.18TIYCh. 1.9 - Prob. 1.19ECh. 1.9 - Prob. 1.20ECh. 1.9 - Prob. 1.21ECh. 1.9 - Prob. 1.22ECh. 1 - Prob. 25PCh. 1 - Prob. 26PCh. 1 - Prob. 27PCh. 1 - Prob. 28PCh. 1 - Prob. 29PCh. 1 - Prob. 30PCh. 1 - Prob. 31PCh. 1 - Prob. 32PCh. 1 - Prob. 33PCh. 1 - Prob. 34PCh. 1 - Prob. 35PCh. 1 - Prob. 36PCh. 1 - Prob. 37PCh. 1 - Prob. 38PCh. 1 - Prob. 39PCh. 1 - Prob. 40PCh. 1 - Prob. 41PCh. 1 - Prob. 42PCh. 1 - Prob. 43PCh. 1 - Prob. 44PCh. 1 - Prob. 45PCh. 1 - Prob. 46PCh. 1 - Prob. 47PCh. 1 - Prob. 48PCh. 1 - Prob. 49PCh. 1 - Prob. 50PCh. 1 - Prob. 51PCh. 1 - Prob. 52PCh. 1 - Prob. 53PCh. 1 - Prob. 54PCh. 1 - Prob. 55PCh. 1 - Prob. 56PCh. 1 - Prob. 57PCh. 1 - Prob. 58P
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- The photoelectron spectrum of HBr has two main groups of peaks. The first has ionization energy 11.88 eV. The next peak has ionization energy 15.2 eV, and it is followed by a long progression of peaks with higher ionization energies. Identify the molecular orbitals corresponding to these two groups of peaks.arrow_forward6. For heteronuclear diatomic molecules, the energy-level diagrams of the molecular orbitals need to be modified via calculation. For both NO and CN', the order of molecular orbitals are similar to that of O,. Write electron configurations of NO and CN including core electrons, starting with o1,'01,*². Which bond is stronger? (hint: bond order)arrow_forwardDraw the molecular orbital energy diagram (like we did in class, not the fancy general chemistry diagrams) for the bond between the nitrogen atom labeled a and the carbon atom labeled b in the following molecule. Clearly indicate which atomic orbitals are interacting, which resulting orbital the electrons are in, and label HOMO, LUMO, bonding and antibonding orbitals, and sigma (o), sigma* (o*), pi (n), and pi* (7*) where appropriate.arrow_forward
- Given that the following MO-energy-level diagram applies to the the diatomic molecular cation BO+, match the letter label of each energy level with the corresponding orbital descriptor. (See attached image!) O2pσ2pσ2s*π2pσ2p*B+2sπ2p*σ2sO2sB+2p Does this diagram display the effect of s-p orbital mixing? YES or NO? Which kind of magnetism would be observed for this cation? paramagnetism diamagnetism What is the bond order for this cation? 0.0, 0.5, 1.0, 1.5, 2.0, 2.5, 3.0, 3.5, 2.0arrow_forward1. Derive the following expression for the bonding and antibonding orbitals of a heteronuclear diatomic molecule consisting of two electrons in a molecular orbital of the form y = CAA + CBB with atomic orbitals A and B. Let aa=HAA, aB=HBB, B=HAB=HBA, SAA-SBB=1, and, as a simplification, let SAB=SBA=S=0 (zero-overlap approximation). Note that the assumption of SAB=SBA=S=0 is used simply to get a more transparent expression. Show that the secular determinant is given by a,-E - E and energies are given by 1/2 2B E̟ = }(a, +a,)±(a,-a,) For B<0, E+ is the lower energy solution.arrow_forward4. Molecular Orbital Theory Let's construct an MO diagram for KrBr*, the krypton bromide cation. Let's focus only on the n=4 valence shell in for both species. a) Which of the two atoms, Kr or Br, has a 4p electrons that are lower in energy? Justify your answer in terms of periodic trends. Also provide experimental evidence for your answer in terms of ionization energies (available online). b) Based on part (a), draw an MO diagram for KrBr*, reflecting the appropriate relative energies of the Kr/Br valence electrons. Connect the orbitals that mix/split with dashed lines. c) Populate the MO diagram with the appropriate number of valence electrons. What is the expected bond order?arrow_forward
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