5. (a) Predict the electron transfer products of the reaction between [Fe(H2O)6]²+ and [Co(NH3)5(NCS)]. (2 marks) (b) Write the electron transfer mechanism and identify the rate determining step of the above reaction in part (a). (c) (7+2 marks) Deduce if the products obtained in part (a) after the electron transfer are labile or inert. (6 marks)

5. (a) Predict the electron transfer products of the reaction between [Fe(H2O)6]²+ and [Co(NH3)5(NCS)]. (2 marks) (b) Write the electron transfer mechanism and identify the rate determining step of the above reaction in part (a). (c) (7+2 marks) Deduce if the products obtained in part (a) after the electron transfer are labile or inert. (6 marks)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter20: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 6Q: Four different octahedral chromium coordination compounds exist that all have the same oxidation...

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Four different octahedral chromium coordination compounds exist that all have the same oxidation state for chromium and have H2O and Cl as the ligands and counterions. When 1 mole of each of the four compounds is dissolved in water, how many moles of silver chloride will precipitate upon addition of excess AgNO3?
Complete the following redox reaction, where X is H2O, NCS-, SCN-, and I-.[Co(NH3)5X]2++ [Cr(H2O)6]2+ → ? Answer the following questions:(a) propose the reaction mechanism, )(b) suggest the order of the rate of reaction, and (c) explain the variation in the rate of reaction
Write the hybridization, shape and magnetic character of [Fe(CN)6]4-.
What type of isomerism is shown by [CO(NH3)5ONO]Cl2? (ii) On the basis of crystal field theory, write the electronic configuration for d4 ion if A0 < P. (iii) Write the hybridization and shape of [Fe(CN)6]3-. (Atomic number of Fe — 26)
Cobalt (II) chloride can form two complexes when dissolved in water: [Co(H2O)6]2+(aq) which is pink in colour, and [CoCl4]2- which is blue. The equilibrium system is
Draw the geometrical isomers of complex [Pt(NH3)2Cl2]. (ii) On the basis of crystal field theory, write the electronic configuration for d4 ion if Δ0 < P. (ii) Write the hybridization and magnetic behaviour of the complex [Ni(CO)4].
State a reason for each of the following situations: (i) Co2+ is easily oxidised to Co3+ in presence of a strong ligand. (ii) CO is a stronger complexing reagent than NH3. (iii) The molecular shape of Ni(CO)4 is not the same as that of [Ni(CN)4]2_.
Give the number of d electrons (n of dn) for the central metal ion in (a) [Cr(H2O)6](ClO3)2; (b) [Mn(CN)6]2-; (c) [Ru(NO)(en)2Cl]Br.
The photographs below (a) show what occurs when a solution of iron(III) nitrate istreated with a few drops of aqueous potassium thiocyanate. The nearly colorlessiron(III) ion is converted to a red [Fe(H2O)5SCN)2+ion. (This is a classic test for thepresence of iron(III) ions in solution.)[Fe(H2O)6]3+(aq) + SCN−(aq) ⇄ [Fe(H2O)5SCN]2+(aq) + H2O(ℓ)(a) As more KSCN is added to the solution, the color becomes even more red.Explain this observation.(b) Silver ions form a white precipitate with SCN−ions. What would you observeon adding a few drops of aqueous silver nitrate to a red solution of [Fe(H2O)5 Explain your observations?
What should happen when the concentration of chloride is increased in a solution containing hexaaquocobalt(II), [Co(H2O)6] 2+ (aq)?
(a) In early studies it was observed that when the complex [Co(NH3)4Br2]Br was placed in water, the electrical conductivity of a 0.05 M solution changed from an initial value of 191 ohm-1 to a final value of 374 ohm-1 over a period of an hour or so. (b) Write a balanced chemical equation to describe the reaction.
The orbital occupancies for the d orbitals of several com-plex ions are diagrammed below. (a) Which diagram corresponds to the orbital occupancy of thecobalt ion in [Co(CN)₆]³⁻? (b) If diagram D depicts the orbital occupancy of the cobalt ionin [CoF₆]ⁿ, what is the value of n? (c) [NiCl₄]²⁻ is paramagnetic and [Ni(CN)₄]²⁻ is diamagnetic.Which diagrams correspond to the orbital occupancies of thenickel ions in these species? (d) Diagram C shows the orbital occupancy of V²⁺ in the octa-hedral complex VL₆. Can you determine whether L is a strong-or weak-field ligand? Explain.