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- Explain why the complex [Fe(H2O)6]3+ has Do = 14,000 cm-1, while [Fe(H2O)6]2+ has Do = 9,350 cm-1.1,Count up the 18-electron rule of the organometallic complex (Ferrocene) using covalent counting method.2. Draw the molecular orbital diagram for B2 and find the bond order?Inorganic Chemistry (i) Define spectrochemical series (ii) Explain the difference between weak-field and strong-field ligands
- 1) What role do the protons play in the transformation of [(SALEN)VO] to [(SALEN)Cl2]? --- Consider the number of anionic charges for all the ligands as well as the charge of the overall complex. Has the oxidation of vanadium changed in this reaction?Copy the structure of EDTA4- from your textbook and circle all six atoms that act as Lewis bases. Why does EDTA4- cease to function as a chelating ligand if acid is added to the solution? pls help asap!!copper complex crystallises straightaway when synthesising but the cobalt complex required the solution to be concentrated and cooled before it is filtered to obtain product. what does this tell you about the realtive solubilities of the copper and cobalt complexes.
- why [Cu(deen)2]X2(X = BF4-, ClO4-and NO3-) show thermochromic behavior, whereas most other bis-diamine Cu(II) complexes (e.g. ethylenediamine) do not exhibit this propertyConstruct an MO correlation diagram for the complex ion[Ni(NH3)6]2+ and populate the orbitals with electrons. Do youexpect p bonding to be important for this complex? Whatfeatures of this diagram correspond to those predicted usingcrystal field theory? What kind of bonding would VB theorypredict for d8 complexes, and how does MO theory accountfor the bonding more accurately, even qualitatively?Consider the [Ir2(dimen)4] 2+ complex. Notice that the dimen ligand is asymmetric. There is also a different, symmetric diisocyano ligand referred to as “TM4” (structure shown to the right) that forms the same sort of binuclear complex that dimen does. Answer the following questions with supporting justification: a. How many geometric isomers (ignore any optical ones) of [Ir2(TM4)4] 2+ are there? b. How many geometric isomers (ignore any optical ones) of [Ir2(dimen)4] 2+ are there? c. In the “twisted” deformational isomer, would you expect [Ir2(TM4)4] 2+ or[Ir2(dimen)4] 2+ to be able to rotate polarized light? Justify your answer.
- What is the expected number of Fe-Febondsper Fe atom in the complex ?Many transition metal complexes are said to follow the “18-electron rule,” meaning they form particularly stable complexes when the metal + ligand electrons contributing to the MOs add up to a total of 18 electrons. a. Use the full MO diagram for an octahedral metal complex with pi-acidic ligands we derived in class to justify why 18-electrons might be particularly stable. b. Use the 18-electron rule to predict which 1st row transition metal would be most likely to form an octahedral M(CO)6 (Note: there is no charge; the metal retains all its electrons.) c. Qualitatively, how would you expect the CO bond to change when it forms this complex? Would it be stronger, weaker, or the same compared to free CO? (Hint: think about what a ? −???? means and what the orbital does from the perspective of the M–CO interaction as well as the C– O interaction).Fill in the blanks : (i) When a ligand has a two-complexing or donor group in its structure, it is said to be————— (ii) ___________are compounds whose colour changes when they bind to a metal ion. (ii) If you double the wavelength, you will observe. ________the energy. (iv) In_____________ titration, we monitor changes in absorbance during the titration to find out the equivalence point. (v) Two liquids are_____________ if they form a single phase when they are mixed in any ratio. (vi) The efficiency of Chromatographic Columns can be described by____________Equation.
