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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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(a) Use the simple one-electron molecular orbital method, including overlap, to calculate the energies of the molecular orbitals of the hydrogen molecule (H2) in terms of α, β and S?
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- An energy level scheme for the orbitals of second row diatomic molecules O, through Ne2 , lists the molecular orbitals in the following order of increasing energy 02 < o'2s < Ozp(z) < T2p(y)- 7T2P(x) < T*2p(y), 7T* 2p(x) < o*2plz) Based on this energy level scheme, how many electrons are there in all of the antibonding molecular orbitals of the F2* ion in its ground state?arrow_forward9A.2 Write the valence bond wavefunction of the o bond in a C-H group of a molecule.arrow_forwardConsider the diatomic molecules O , 0",0; and O;, where O; corresponds to the neutral O2 molecule in its lowest excited state. Order the molecules by their expected bond length according to molecular orbital theory (from shortest to longest bond length). In your work, also write down the electron configurations for each of the diatomic molecules.arrow_forward
- 6. 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_forwardIdentify the g or u character of bonding and antibonding π orbitals formed by side-by-side overlap of p atomic orbitals.arrow_forward
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