(1) (a) Draw an energy level diagram showing the ground state electronic struc- ture of each of the following diatomics: H₂, N2, O2, F2, and Ne₂. (b) Use the above diagram to predict the bond order of each of these diatomics. (c) Use the same procedure to predict the bond order of C and O
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- (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.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 muchIf an electron is removed from a fluorine molecule, an F+2molecular ion forms.(a) Give the molecular electron configurations for F2 and F+2 (for the MOs constructed from valence AOs).(b) Give the bond order of each species.(c) Predict which species should be paramagnetic.(d) Predict which species has the greater bond dissociation energy.
- When one electron is added to an oxygen molecule, a superoxide ion (Oz) is formed. The addition of two elec- trons gives a peroxide ion (Oź ). Removal of an electron from O, leads to Ož. (a) Construct the correlation diagram for Oz. (b) Give the valence electron configuration for each of the following species: Ož, O2, 0z, 03 . (c) Give the bond order of each species. (d) Predict which species are paramagnetic. (e) Predict the order of increasing bond dissociation energy among the species.Are these statements true or false? Correct any that are false.(a) Two bonds comprise a double bond.(b) A triple bond consists of one bond π and two bonds σ.(c) Bonds formed from atomic sorbitals are always bonds.(d) A π bond restricts rotation about the σ-bond axis.(e) A π bond consists of two pairs of electrons.(f) End-to-end overlap results in a bond with electron density above and below the bond axis.Consider the Lewis structure shown below.(a) Does the Lewis structure depict a neutral molecule or anion? If it is an ion, what is the charge on the ion? (b) What hybridizationis exhibited by each of the carbon atoms? (c) Arethere multiple equivalent resonance structures for the species?(d) How many electrons are in the p system of the species?
- (A)Write the Hückel Hamiltonian matrix for benzene. (B) The pictures below represent a top view of the π molecular orbitals for benzene. They are labeled from A to F, in no order. Place the labels A, B, C, etc., in the boxes according to their energy. SHOW THE NODES. (B)N2 and CN' are both isoelectronic. (i) Draw the molecular orbital diagram for N2 and CN molecules. (ii) Explain why CN is a toxic substance but N2 isn't. (iii) N2(g) is an inert gas that is suitable for a wide range of application. Would you expect N2" to be a stable diatomic species in the gaseous state? Explain your answer.The ground-state electron configuration of He; is (o,1s)'(0,1s)' . Calculate the bond order of Hez. (A) 3/2 (B) 1/2 (С) 1 (D) -1/2
- 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.Calcium carbide, CaC2,contains the acetylide ion, C22-.Sketch the molecular orbital energy'level diagram for the ion and the electron dot strucure. (a) How many net σ and π bonds does the ion have? (b) What is the carbon-carbon bond order? (c) Compare the valence bond and MO pictures with regard to the number of σ and π bonds and the bond order. (d) How has the bond order changed on adding electrons to C2 to obtain C22-? (e) Is the C22- ion paramagnetic?Acetylene (C2H2) has a tendency to lose two protons (H+) and form the carbide ion (C22−), which is present in a number of ionic compounds, such as CaC2 and MgC2. (a) What is the bond order of the carbide dianion C22−? (b) For comparison, what is the bond order of C2?