Answered: (a) State the Jahn-Teller Theorem. (b)… | bartleby

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter21: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 1ALQ

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(a)
State the Jahn-Teller Theorem.
(b)
Show how Jahn-Teller distortion would affect the geometry of [Cu(OH2)6]²+
Illustrate your answer with suitable structure diagrams.

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(a) What is the range in electronegativity across the first (3d)transition series? (b) What is the range across Period 4 of main-group elements? (c) Explain the difference.
Predict the products of each of the following reactions and then balance the chemical equations.(a) Fe is heated in an atmosphere of steam.(b) NaOH is added to a solution of Fe(NO3)3.(c) FeSO4 is added to an acidic solution of KMnO4.(d) Fe is added to a dilute solution of H2SO4.(e) A solution of Fe(NO3)2 and HNO3 is allowed to stand in air.(f) FeCO3 is added to a solution of HClO4.(g) Fe is heated in air.
Give the electron configuration and the number of unpaired electrons for: (a) Cr3+; (b) Ti4+; (c) Co3+; (d) Ta2+.
Basic solutions of Na4XeO6 are powerful oxidants. What mass of Mn(NO3)2•6H2O reacts with 125.0 mL of a 0.1717 M basic solution of Na4XeO6 that contains an excess of sodium hydroxide if the products include Xe and solution of sodium permanganate?
Give the oxidation state of the metal for each of the following oxides of the first transition series. (Hint: Oxides of formula M3O4 are examples of mixed valence compounds in which the metal ion is present in more than oneoxidation state. It is possible to write these compound formulas in the equivalent format MO∙M2O3, to permit estimation of the metal’s two oxidation states.)(a) Sc2O3(b) TiO2(c) V2O5(d) CrO3(e) MnO2(f) Fe3O4(g) Co3O4(h) NiO(i) Cu2O
(a) Calculate the number of unpaired electrons in the following gaseous state ions: Mn2+, Cr3+, V3+ and Fe2+ which one of these in the most stable in aqueous solutions? (At. nos. V = 23, Cr = 24, Mn = 25, Fe = 26) (b) Explain the following observations: (i) The transition metal ions are usually coloured in aqueous solutions. (ii) Cu(I) is not stable in an aqueous solution. (iii) The highest oxidation state of a transition metal is exhibited in its oxide or fluoride.
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.
Identify the oxidation state for vanadium in [VO2(H2O)4]+1.
Describe/draw the formation of bond in the following compounds: (i) CaCl2 (ii) K2O (iii) O2
One of the steps for refining silver involves converting silver into dicyanoargenate(I) ions: 4Ag(s) + 8CN−(aq) + O2(g) + 2H2O(l) ⟶ 4[Ag(CN)2]−(aq) + 4OH−(aq)Explain why oxygen must be present to carry out the reaction. Why does the reaction not occur as: 4Ag(s) + 8CN−(aq) ⟶ 4[Ag(CN)2−(aq)?
Using the periodic table to locate each element, write the electron configuration of (a) V; (b) Y; (c) Hg.
Assign a reason for each of the following observations:(i) The transition metals (with the exception of Zn, Cd and Hg) are hard and have high melting and boiling points.(ii) The ionization enthalpies (first and second) in the first series of the transition elements are found to vary irregularly.

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