3a) The nitrosyl ion, NO*, is a very rare case of a cationic ligand that can function as a Lewis base. Drawthe Lewis structure of this ligand under consideration of the VSEPR rules and indicate any formalcharges 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.

(3a)Step 1: Step 2: Step 3: (3b)Step 1: Step 2:

Answered: 3a) The nitrosyl ion, NO*, is a very…

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider bis(ethylenediamine) copper(ii) complex ion, Cu(en)22+ : A ) Explain the bond formation in this ion in terms of lewis acid- base theory. B) Sketch the ion with some drgree of three- dimensional clarity. Indicate the structure of the ion.
The ligand bpy forms complexes with Ru³+ and Ru²+. The standard potential of the couple is +1.26 V. Does bpy bind preferentially to Ru³+ or Ru²+? Why? [Ru(bpy)3]³+/[Ru(bpy)3]²+ 3+
Denticity Denticity is the number of atoms in a ligand that bind to a central atom in a coordination complex. H H For example, ethylene diamine (shown on the right) has two nitrogen atoms with lone pairs that can both bind to a metal. This ligand is bidentate. N: Identify the number of atoms in each ligand that can donate a lone pair. N: O monodentate O not a ligand O bidentate O bidentate O not a ligand O monodentate CH3 O bidentate O not a ligand O monodentate OH O bidentate O monodentate O not a ligand
A) Using a cobalt (III) ion as the central metal atom, and with chloride ions (Cl-) and ammonia (NH3) molecules as the ligands, draw both isomers of the coordination complex that will exhibit fac/mer isomerism. B) Using a platinum (II) ion as the central metal atom, with chloride ions and ammonia molecules as the ligands, draw both isomers of the coordination complex that will exhibit cis/trans isomerism. Platinum (II) forms four coordinate bonds.
The compound [Fe(H2O)6]SO2 has a pale green color. The compound K4[Fe(CN)6] has a bright yellow color. Which of the following statements are NOT true? Select the correct answer below: A) The compound K4[Fe(CN)6] absorbs higher energy light. B) H2O produces a stronger ligand field than CN−. C) The compound K4[Fe(CN)6] is likely a low-spin complex because it contains strong-field ligands. D) The compound [Fe(H2O)6]SO2 is likely a high-spin complex because it contains weak-field ligands.
The cyanide anion CNis a very good ligand towards metal ions.Represent the Lewis formula of the cyanide ion, and by which atom does the cyanide anion coordinates to a metal ion?
Transition metal complexes are highly likely to be colored because of a) the size of the energy gap within the d orbitals and the number of electrons. In ruby, the red color of ruby is attributed to a small amount of Cr³* substituting into Al2O3 which is made up of shared AIO, octahedra. Provide a hypothesis for the origin of the red color observed in ruby. Red pigments tend to be rare. If you had to design a new material that b) had an approximate bandgap that would absorb green, what ideas do you need to employ to find a new semiconductor that does not contain Cd, Hg or Pb as one of the components (see last lecture for ideas).
Cr(aq) + 3 e Cr(s) Zn²(aq) + 2 e → Zn(s) 2 H₂O() +2 e → H₂(g) + 2 OH(aq) Mn2(aq) + 2 e A(an) + 3 e Mn(s) Al(s) 7. All of the following statements concerning ligand field theory are true EXCEPT A. in low-spin complexes, electrons are concentrated in the day, dys, and dr orbitals. B. in an isolated atom or ion, the five d orbitals have identical energy. C. low-spin complexes contain the maximum number of unpaired electrons. D. the crystal field splitting is larger in low-spin complexes than high-spin complexes. E. the energy difference between d orbitals often corresponds to an energy of visible light. 8. All of the following complexes will be colored (in the visible) EXCEPT A. [Co(en)]2+ B. [Fe(CN)6] C. [Ni(H₂O)]²+ D. [Cd(NH3)4]2+ 9. A positron has a mass number of a(n) a. 0; 1+; proton b. 1; 2+; proton c. 0; 1+; electron d. 1; 2+; electron e. 0; 0; proton -0.76 -0.83 -1.18 -1.66 a. [Cr(CO)6]C13 b. [Cu(OH)4(NH3)2] c. K4[Mn(CN)6] d. [Pt(en)3] (NO3)4 e. [Pt(NH3)2(OH₂)CIJ3PO4 10. In which…

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS