For N₂ and N₂*, a) b) c) d) Construct a MO diagram. State the magnetic property Calculate the bond order Describe the differences in bond strength and bond length.
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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?1) For N2 and N2*, molecule: a) Construct a MO diagram. b) Calculate the bond order. c) State the magnetic property d) Write the electronic configuration. e) Describe the differences in bond strength and bond length.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.
- 2. Draw MO energy level diagrams for each of the following diatomic molecules are molecular ions. All contributing atomic orbitals and the resulting molecular orbitals must be labeled properly showing the electrons (as arrows) in the atomic orbitals and in the molecular orbitals. All orbitals should be drawn to show their relative energy relationships. Calculate the bond order for each and label each as either diamagnetic or paramagnetic. (a) BO‒ (b) CN (c) FCl (d) Cl2‒3) Draw the complete MO diagram and write out the complete MO configuration for N₂* Identify (a) the bond order, (2) whether it is paramagnetic or diamagnetic, and (3) is the bond shorter or longer than N₂ (neutral)State whether each of the following atomic orbital combinations will result in a sigma (σ), pi (π), or an orthogonal interaction. Always bear in mind that the accepted internuclear axis is always the z-axis. (c) dxz with dxy (d) dxz with dxz
- What is the primary difference between valence bond theory (VB) and molecular orbital theory (MO)? A) VB determines the summation of mixed wave functions as hybrid orbitals; MO determines the sum of atomic orbital energy as energy level diagrams. B) VB determines the summation of mixed wave functions as energy level diagrams; MO determines the sum of atomic orbital energy as hybrid orbitals. C) MO determines the summation of mixed wave functions as energy level diagrams; VB determines the sum of atomic orbital energy as hybrid orbitals. D) MO determines the summation of mixed wave functions as hybrid orbitals; VB determines the sum of atomic orbital energy as energy level diagrams.(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.1. MO diagrams for ions: Molecule orbital diagrams can also be used to predict the bond orders of not-so- common molecules and ions. (a) On the blank MO diagrams below, draw complete molecular orbital energy-level diagrams for O₂ and O₂. Predict the bonds orders of these molecules. (b) Repeat the exercise above for N₂ and N₂". (c) Use valence bond theory to draw Lewis structures of the four ions above. What bond order do these Lewis structures suggest? Compare these bond orders with the predictions of MO theory and discuss the similarities and differences. 1113 2p 12 2s 1 1 1 2p 14 2s 2p 2p A
- ne: For the following species: O2, O7, 0 Rank the following from least to greatest according to MO theory. (a) bond order (b) bond length (c) bond energy (d) magnetic characterConsider the valence bond description of the covalent bonding in N2H2.(a) Draw the Lewis structure for N2H2. [3 pts](b) Identify the hybridization scheme for the two N atoms. [3 pts](c) Using the same techniques shown in class, sketch the valence bond model for N2H2I wonder (d) below. Carbon monoxide is produced by incomplete combustion offossil fuels.(a) Give the electron configuration for the valence molecular orbitals of CO. The orbitals have the same energyorder as those of the N2 molecule.(b) Do you expect CO to be paramagnetic or diamagnetic?(c) What is the bond order of CO? Does this match thebond order predicted by the electron-dot structure?(d) CO can react with OH- to form the formate ion,HCO2-. Draw an electron-dot structure for the formateion, and give any resonance structures if appropriate. Thanks:)