课程名称︰无机化学一 课程性质︰系定必修 课程教师︰王瑜 开课学院：理学院 开课系所︰化学系 考试日期（年月日）︰2008/12/10 考试时限（分钟）：3.4节 试题 : 1. compare the confing in O2 . O2-,(O2)2-. Include Lewis structures, molecular orbital (MO) structures, bond lengths, bond orders , and bond energies in your comparison. Try to correlate the Lewis structure and MO electron pairs in the case of O2 2. Prepare MO energy level diagrams for the CN- and N2, Which are iso-electronic. a. what is the respective bond order? Describe each bond with sketches. b Are their any lone pairs ? if so,where are they located? c. Illustrate the highest occupied MO(HOMO) and the lowest unoccupied MO(LUMO) for both molecules. d. Which MO of CN- would you expect to interact strongly with a 1s orbital of H to form a neutral molecule HCN? e. Why CN- is a strong ligand but N2 is not. 3.For Diborane B2H6 . what are the possible hybrid orbitals for B? Explain the B-H-B bond as three centered bond in terms of MO description. 4 Describe the MO diagram for CO2 . Use the same diagram to explain why the geometry of O3 is no longer linear? 5.[Co(H2O)6]3+ is a strong oxidizing agent what will oxidize water, but [Co(NH3)6]3+ is a stable in aqueous solution, explain the difference. Both are low spin complexes with Δof 16750 and 24000 cm-1 respectively. 6. construct the hybrid orbital of metal ion (M) in ML5 in square pyramidal and trigonal bipyramidal geometries; work out the possible σand Π bond interactions between M and L .Using angular overlap model(AOM) determine the energies of d-orbital for M in each geometry, where the ligands act as a. σ donor only b. σ donor and Π donor c. σ donor and Π acceptor compare the ligand field stabilization energy(LFSE) in terms of eσ and eΠ for d3-d8 between 2 geometries. -- --

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