Mn, Fe, and Co in the +2 and +3 oxidation states allform hexaaquacomplexes in acidic aqueous solution. Thereduction reactions of the three species are representedschematically below, where the water ligands are notshown for simplicity. It is an experimental fact from elec-trochemistry that Mn2+ and Co²+ are more easily reducedthan Fe3+; that is, they will more readily accept an elec-tron. Based on the electron configurations of the ionsinvolved, explain why Fe³+ is harder to reduce than Mn2+and Co²+.Mn3+ + e – Mn²+Fe* + e –→ Fe²+Co³++ e → Co²+

The process by which an atom gain an electron or an electron pair is called reduction. The electrons…

Answered: Mn, Fe, and Co in the +2 and +3…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter8: Bonding In Transition Metal Compounds And Coordination Complexes

Section: Chapter Questions

Problem 34P

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A 3.03-g petroleum specimen was decomposed by wet ashing and subsequently diluted to 500 mL in a volumetric flask. Cobalt was determined by treating 25.00-mL aliquots of this diluted solution as follows: Assume that the Co(II)-ligand chelate obeys Beer’s law, and calculate the percentage of cobalt in the original sample.
Nickelocene is an example of another meallocene. It is paramagnetic with two unpaired electrons. Rationalise this and suggest a bonding scheme, which accounts for it. Do start with the symmetry and the molecular orbitals of the Cp- ligand.
Nickelocene is paramagnetic with two unpaired electrons. Rationalise this and suggest a bonding scheme, which accounts for it. Do start with the symmetry and the molecular orbitals of the Cp- ligand.
Using periodic trends, crystal structures, valence states, etc., explain the complex spectrum of electronic properties of transition metal compounds (e.g. from TiO to NiO), and describe the main factors that affect the electronic properties, or favour electronic conduction, of inorganic materials. As a specific case of the above question, predict and account for the differences in electronic properties between (a) TiO2 and TiS2, and (b) TiO2 and VO2.
Nickelocene is paramagnetic with two unpaired electrons. Why is it so? Rationallise it and back up your answers and suggest a bonding scheme, which accounts for the two unpaired electrons. Do start with the symmetry and the molecular orbitals of the Cp- ligand.
Explain in detail π backbonding using the molecular orbitals of CO and a d-transition metal. How does this influence Infrared Spectroscopy and explain how the bond order for the C-O bond changes and how the bond order for the metal-ligand bond changes. Provide pictures and explanations. (Inorganic Chemistry)
In general, would you expect EDTA4- to coordinate to transition metal ions more or less strongly than ethylenediamine does? Justify your answer with a reason other than the different charges on the two ligands.
There are two different crystalline vanadium fluorides, in both the V is in an environment octahedral. One is blue and the other is yellow. The oxidation state of vanadium in one of them is +2, and on the other, +3. Deduce, from the different crystal field doublings, which is which (No numerical calculation necessary, use spectrochemical series and spectrum electromagnetic and / or colored circle to justify your answer).
1. Account for the fact that [SiF6]-2 is a well-known species, while the corresponding [CF6]-2 does not exists. 2. Arrange the following oxides K2Cr2O7, Cr2O3 and CrO in order of increasing oxidizing power. Write the oxidation states of Cr in each compound. 3. Which is more easily hydrolysed CCl4 or SiCl4? Explain your answer.
(a) Which metal in the first transition series (3d series) exhibits +1 oxidation state most frequency and why?(b) Which of the following cations are coloured in aqueous solutions and why?SC3+, V3+, Ti4+, Mn2+.(At. nos. Sc = 21, V = 23, Ti = 22, Mn = 25)
For problem 2, I have to assign oxidation states for transition metals by drawing the lewis structure with all the sigma bonds, rmeoving all the ligands on their closed shell configuration and noting the formal charge, and accounting for all the ligand charges, where oxidation number = molecular charge - sum of ligand charges.I am unsure how to identify Lewis acids. How to solve Problem 7?
Is it posible to remove 99% of 1.0 μM CuY2- impurity (by reduction to solid Cu) from a 10.0 mM CoY2- solution at pH 4.0 without reducing any cobalt? Here, Y (actually, Y4-) is EDTA and the total concentration of free EDTA is 10.0 mM. Hint: Concepts of Equilibrium of EDTA Complex Formation are involved in the solution of this problem. Standard reduction potentials to use in this problem are:CuY2- + 2e- ➙ Cu(s) + Y4- E°= -0.216 VCo2+ + 2e- ➙ Co(s) E°= -0.282 V.

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