課程名稱︰無機化學一
課程性質︰系定必修
課程教師︰王瑜
開課學院：理學院
開課系所︰化學系
考試日期（年月日）︰2008/12/10
考試時限（分鐘）：3.4節
試題 :
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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