4610ex2practice - 1 through d 8 . If a choice of spin is...

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1 Explain, using molecular orbital theory terms why the 18 electron rule is so important for organometallic compounds, yet it is not as important for classical “Werner” type complexes. 2 In the molecular orbital diagram of SF 4 , show which atomic orbitals participate in bonding, which may not participate in bonding and which can mix. Use Group Theory. You do not need to draw the MO diagram. (20 points) 3 In the SF 4 molecule above, show which of the S-F vibrations are IR active and which are Raman active. 4. Construct a molecular orbital diagram for the trigonal planar molecule BH 3 (D 3 h) and for the trigonal pyramidal molecule NH 3 . You do not have to show me what the symmetrized Group Orbitals look like. 5. Calculate the Crystal Field Stabilization Energy the metal complexes d
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Unformatted text preview: 1 through d 8 . If a choice of spin is evident, do the low spin case only. 6. For the compound MX4, which has Td, coordination, determine all the stretching vibrations. Then determine which are IR active and Raman active. 7. For the compound MX5, which has D3h coordination, determine which orbitals participate in bonding. Now do the same thing for MX4, which is see saw shaped (C2v coordination). 8. Tell me about crystal field theory. Describe the theory in as much detail as possible. You need not go into tetragonal distortions. 9. What do the terms labile and inert mean. Is this the same as stable and unstable? Using molecular orbital arguments, why are the complexes d1, d2 and d4 high spin labile while d3, d4 low spin and d6 low spin, inert?...
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