1. Below is a molecular orbital diagram for a generic metallocene. Based on this, contrast the metal carbon bond lengths in chromocene [Cr(CsHs)2], ferrocene [Fe(CsHs)2] and nickelocene [Ni(CsHs)2]. Which would you expect to be a reductant, which is an oxidant and which is stable? Justify your answer. M MCP 2 Cp equ ezg 4p azu ezgi ezu azu etu ezu 45 aig 3d alg eig 20 equ 19 ezg 19 1gazu

9. Name the following compounds. a. Ni(CO)4 b. Naz[Co(H₂O)2(OH)4] c. [Ag(NH3)2] Br d. [Co(NH3)4C1]SO4 g. [Ni(NH3)4(H₂O)2](NO3)2

3a) The nitrosyl ion, NO*, is a very rare case of a cationic ligand that can function as a Lewis base. Draw the Lewis structure of this ligand under consideration of the VSEPR rules and indicate any formal charges on the constituent atoms. 3b) How many electrons does the NO* ligand contribute on the ionic model and the neutral model, respectively? Assume that the Metal-N-O bonding angle is 180° upon coordination.

Draw appropriate energy diagrams and determine all possible numbers of unpaired electrons in compounds of the following ions within an octahedral crystal field: (a) Mn2 +, (b) Co3 +, (c) Ni2 +, (d) Fe3 +

Write the formula for diaquadibromoplatinum (II). C [Pt(H2O)2Br2]2 C [Pt(H2O)2]Br2*1 C [Pt(H2O)2]Br2 C [Pt(H2O)2]Br22 C (Pt(H2O)2Br2] C PE(H,O),Bra]*1

[Fe(H2O)6]2+,  calculate the bond order

Consider the reactions 1. [Cr(H2O)6]** + [C©CI(NH3)s]* → [Co(NH3)s(H2O)]²* + [CrCl(H2O)s]** 2. [Fe(CN)6]* + [Mo(CN)s]-→ [Fe(CN)6]³¯ + [Mo(CN)8]* Which one of the following is the correct statement? (i) Both involve an inner sphere mechanism (ii) Both involve an outer sphere mechanism (iii) Reaction 1 follows inner sphere and reaction 2 follows outer sphere mechanism (iv) Reaction 1 follows outer sphere and reaction 2 follows inner sphere mechanism (A) i (B) ii (C) iv (D) ii

6. A mixture contains at least one of the ions in the silver group (Ag*, Hg²*, Pb²+). Read the following procedure and determine which ions are present. Cold 6M HCl was added to the mixture producing a white precipitate. Hot water was then added and the solution was stirred, and the supernatant decanted to isolate a white precipitate after centrifugation. Sulfuric acid was added to one portion of the supernatant and potassium chromate was added to a second portion of the supernatant, but no precipitates formed. The isolated white precipitate was mixed well with 4 drops of concentrated ammonia. The resulting solution was centrifuged. The supernatant was decanted to show the presence of a grayish-black precipitate. To the supernatant, concentrated nitric acid was added dropwise until blue litmus paper added turned red and a white precipitate was present.

Give the electron configuration and the number of unpaired electrons for: (a) Cr3+; (b) Ti4+; (c) Co3+; (d) Ta2+.

Consider the [VII(H2O)6]2+ ion. Explain why there are this number of bands and not more or less, which might be expected (i.e., which sets of electronic transitions give rise to these bands).