Part A Using the molecular orbital energy ordering for second-period homonuclear diatomic molecules in which the 2p orbitals lie at lower energy than the 2p, draw MO energy diagrams for a molecule or ion with four valence electrons. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Not all targets will be filled. G2 G1 吃 G2 G2 G1 OSP G2 G1 G2 G2 G1 1L Submit Request Answer G2 G1 G2 G1 Reset Help

Part A Using the molecular orbital energy ordering for second-period homonuclear diatomic molecules in which the 2p orbitals lie at lower energy than the 2p, draw MO energy diagrams for a molecule or ion with four valence electrons. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Not all targets will be filled. G2 G1 吃 G2 G2 G1 OSP G2 G1 G2 G2 G1 1L Submit Request Answer G2 G1 G2 G1 Reset Help

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter6: Quantum Mechanics And Molecular Structure

Section: Chapter Questions

Problem 39P: The photoelectron spectrum of HBr has two main groups of peaks. The first has ionization energy...

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The B2 molecule is paramagnetic; show how this indicates that the energy ordering of the orbitals in this molecule is given by Figure 6.18a rather than 6.18b.
The MO of the ground state of a heteronuclear diatomicmoleculeAB is mol=CAA+CBB If a bonding electron spends 90% of its time in an orbital A on atom A and 10% of its time in B on atom B, what are the values of CA and CB ? (Neglect the overlap of the two orbitals.)
Considering only the molecular orbitals formed by combinations of the 2s atomic orbitals, how many molecular orbitals can be formed by 1000 Li atoms? In the lowest energy state, how many of these orbitals will be populated by pairs of electrons and how many will be empty?
Solid sulfur normally consists of crystals of S8 molecules, but when heated strongly, the solid vaporizes to give S2 molecules (among other molecular species). Describe the bonding in S2 in molecular orbital terms, assuming the orbitals are analogous to those of the preceding period. What would you expect to happen to the sulfur sulfur bond length if two electrons were added to give the S22 ion? What would you expect to happen to the bond length if, instead, two electrons were taken away to give S22+?
The existence of compounds of the noble gases was once a great surprise and stimulated a great deal of theoretical work. Sketch the molecular orbital energy level diagram for XeF and deduce its ground state electron configurations. Is XeF likely to have a shorter bond length than XeF+?
1. 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.
Like many of the molecules we have studied in this class, propene (structure shown below) can be thought of as a particle in a box. There are three t-electrons. Since I can put two electrons in each energy level, the highest-energy electron is in the n = 2 state (the HOMO). What does the wave for this electron look like? n = 3 lowest unoccupie molecular orbital (LUMO) n = 2 highest occupiedi molecular orbital (НОМО) . n = 1 Select one: Оа. O b. О с. O d. None of these shapes are right.
Huckel theory: All atomic orbital coefficients in the lowest energy MO (Ψ1) should have the same value – explain why?
Consider a ring system made up of 8 atoms (each one contributing a p atomic orbital to make 8 pi molecular orbitals). If the system is filled with 6 orbitals containing single, electrons, there will 6 orbitals containing pairs of electrons and 1 unpaired electrons. Hint: Use a Frost Circle. Use numbers rather than text for your answers.
The molecule PtCl 2 - is an important square planar starting material in synthetic inorganic chemistry. Using the p orbitals of Cl as the basis find the irreducible representations of the p orbitals and indicate which orbitals could possibly overlap with any of the orbitals on Pt . Assume that the pz orbitals on Cl are orientated in the same direction as the principle rotation axis, px orbitals are pointed at the Pt , and the py orbitals are orthogonal to the px orbitals. Show the characters of each orbital and identify which orbitals on Pt would match from a pure symmetry standpoint.
1. Draw the MO diagram for HBr. The orbital potential energies for the 4s and 4p of Br are -18.65 ev and -12.49ev, respectively. Recall that the H 1s is -13.61ev.
What is the ground state electron configuration for Be+2? What is the bond order for Be+2?

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