The ground-state electron configuration of the H; molec- ular ion is (og15)'. (a) A molecule of H absorbs a photon, promoting the electron to the os molecular orbital. Predict what happens to the molecule. (b) Another molecule of H absorbs even more energy promoting the electron to the o,2, molecular orbital. Predict what happens to this molecule.

The ground-state electron configuration of the H; molec- ular ion is (og15)'. (a) A molecule of H absorbs a photon, promoting the electron to the os molecular orbital. Predict what happens to the molecule. (b) Another molecule of H absorbs even more energy promoting the electron to the o,2, molecular orbital. Predict what happens to this molecule.

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 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.
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.
(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?
Indicate whether each statement is true or false. (a) s orbitalscan only make s or s* molecular orbitals. (b) The probabilityis 100% for finding an electron at the nucleus in a p* orbital.(c) Antibonding orbitals are higher in energy than bondingorbitals (if all orbitals are created from the same atomic orbitals).(d) Electrons cannot occupy an antibonding orbital.
(a) Dihydrogen cation H2+ is commonly found in interstellar space. It can be generated by ionization of dihydrogen molecule H2. What electromagnetic radiation can be used to generate the H2+ cation? (b) Construct an energy level diagram for the molecular orbitals of the H2+ cation. What is the bond order of the HH bond in the H2+ cation? (c) Suggest a spectroscopic method for differentiation of H2 gas and the H2+ cation. Explain your answers.
9. Resonance and hybridization questions. (a) Write valence bond wavefunction for the resonance hybrid HF + H'F (allow for different contributions for each structure). (b) Write valence bond wavefunction for the resonance hybrid CO + Co* + C*o' (allow for different contributions for each structure).
4. (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 a, ß and S? (b) Calculate & given that a = -13.6 eV, that S = 0.6, and that the lowest UV absorption energy is 12 eV. (c) Determine the ionisation energy of the bonding molecular orbital in H₂ ? [6 marks]
Indicate whether each statement is true or false. (a) s orbitalscan only make σ or σ* molecular orbitals. (b) The probabilityis 100% for finding an electron at the nucleus in a π* orbital.(c) Antibonding orbitals are higher in energy than bondingorbitals (if all orbitals are created from the same atomic orbitals).(d) Electrons cannot occupy an antibonding orbital.
Consider a N2 molecule in its first excited electronic state. (a) Identify the molecular orbitals involved and sketch a diagram to show the transition (b) Compare the bond order and bond length of N2* with N2, where the asterisk denotes the excited molecule. (c) Is N2* diagmagnetic or paramagnetic? (d) When N2* loses its excess energy and converts to the ground state N2, it emits a photon of wavelength 470 nm. Calculate the energy difference between these levels. thank you so much
Many primary amines, RNH2, where R is a carbon-containing fragment such as CH3, CH3CH2, and so on, undergo reactions where the transition state is tetrahedral. (a) Draw a hybrid orbital picture to visualize the bonding at the nitrogen in a primary amine (just use a C atom for “R”).
Dinitrogen difluoride, N₂F₂, is the only stable, simple inor-ganic molecule with an N=N bond. The compound occurs incisand transforms.(a) Draw the molecular shapes of the two forms of N₂F₂.(b) Predict the polarity, if any, of each form.
Consider the molecule BF3. (a) What is the electron configurationof an isolated B atom? (b) What is the electron configurationof an isolated F atom? (c) What hybrid orbitalsshould be constructed on the B atom to make the B–F bondsin BF3? (d) What valence orbitals, if any, remain unhybridizedon the B atom in BF3?