(a) The ionization energy of molecular hydrogen (H2) is greater than that of atomic hydrogen (H), but that of molecular oxygen (O2) is lower than that of atomic oxygen (O). Explain. (Hint: Think about the stability of the molecular ion that forms in relation to bonding and antibonding electrons.) (b) What prediction would you make for the relative ion- ization energies of atomic and molecular fluorine (F and F2)?

(a) The ionization energy of molecular hydrogen (H2) is greater than that of atomic hydrogen (H), but that of molecular oxygen (O2) is lower than that of atomic oxygen (O). Explain. (Hint: Think about the stability of the molecular ion that forms in relation to bonding and antibonding electrons.) (b) What prediction would you make for the relative ion- ization energies of atomic and molecular fluorine (F and F2)?

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 67AP: The B2 molecule is paramagnetic; show how this indicates that the energy ordering of the orbitals in...

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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.
Three biological ly important diatomic species. eitherbecause they promote or inhibit life. are (a) CO. (b) NO. and(c) CN-. The first binds to haemoglobin. the second is a neurotransmitter. and the third interrupts the respiratory electrontransfer chain. Their biochemical action is a reflection of theirorbital structure. Deduce their ground-state electron configurations. For heteronuclear diatomic molecules. a good firstapproximation is that the energy level diagram is much thesame as for homonuclear diatomic molecules
(a) Sketch the molecular orbitals of the H2- ion and draw itsenergy-level diagram. (b) Write the electron configuration ofthe ion in terms of its MOs. (c) Calculate the bond order inH2-. (d) Suppose that the ion is excited by light, so that anelectron moves from a lower-energy to a higher-energy molecularorbital. Would you expect the excited-state H2- ion to bestable? (e) Which of the following statements about part (d) is correct: (i) The light excites an electron from a bonding orbitalto an antibonding orbital, (ii) The light excites an electronfrom an antibonding orbital to a bonding orbital, or (iii)In the excited state there are more bonding electrons thanantibonding electrons?
The photoelectron spectrum of HBr has two main groupsof peaks. The first has ionization energy 11.88 eV. Thenext peak has ionization energy 15.2 eV, and it is followedby a long progression of peaks with higher ionizationenergies. Identify the molecular orbitals corresponding tothese two groups of peaks.
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Three biological ly important diatomic species. either because they promote or inh ibit life. are (a) CO, (b) NO, and (c) CN-. The first binds to haemoglobin. the second is a neurotransmitter, and the third interrupts the respiratory electrontransfer chain. Their biochemical action is a reflection of their orbital structure. Deduce their ground-state electron configurations. For heteronuclear diatomic molecules. a good first approximation is that the energy level diagram is much the same as for homonuclear diatomic molecules.
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Is the electron density consistentwith equal contributions from the tworesonance structures for O3? Explain.
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(a) Predict the geometry of the SbCl52- ion, using theVSEPR method.(b) The ion SbCl63- is prepared from SbCl52-by treatment with Cl2. Determine the steric number of thecentral antimony atom in this ion, and discuss theextension of the VSEPR theory that would be neededfor the prediction of its molecular geometry.
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Consider the H2+ ion. (a) Sketch the molecular orbitals ofthe ion and draw its energy-level diagram. (b) How manyelectrons are there in the H2+ ion? (c) Write the electronconfiguration of the ion in terms of its MOs. (d) What isthe bond order in H2+? (e) Suppose that the ion is excitedby light so that an electron moves from a lower-energy toa higher-energy MO. Would you expect the excited-stateH2+ ion to be stable or to fall apart? (f) Which of the followingstatements about part (e) is correct: (i) The light excitesan electron from a bonding orbital to an antibonding orbital,(ii) The light excites an electron from an antibonding orbitalto a bonding orbital, or (iii) In the excited state there are morebonding electrons than antibonding electrons?