Amino acids, such as glycine (gly), form complexes with the trace metal ions found in the bloodstream. Glycine, whose structure is shown here, acts as a bidentate ligand coordinating with the nitrogen atom and one of the oxygen atoms. но H2N-Ç-C-OH Draw all the possible isomers of: a. square planar [Ni(gly), c. octahedral (Fe(gly),) b. tetrahedral (Zn(gly),

Amino acids, such as glycine (gly), form complexes with the trace metal ions found in the bloodstream. Glycine, whose structure is shown here, acts as a bidentate ligand coordinating with the nitrogen atom and one of the oxygen atoms. но H2N-Ç-C-OH Draw all the possible isomers of: a. square planar [Ni(gly), c. octahedral (Fe(gly),) b. tetrahedral (Zn(gly),

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter20: Chemistry Of Selected Transition Elements And Coordination Compounds

Section: Chapter Questions

Problem 121QRT: The glycinate ion (gly) is H2NCH2CO2. It can act as a ligand coordinating through the nitrogen and...

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a. In the absorption spectrum of the complex ion Cr(NCS)63, there is a band corresponding to the absorption of a photon of light with an energy of 1.75 104 cm-1. Given 1 cm1 = 1.986 1023 J, what is the wavelength of this photon? b. The CrNC bond angle in Cr(NCS)63 is predicted to be 180. What is the hybridization of the N atom in the Ncs- ligand when a Lewis acid-base reaction occurs between Cr3+ and NCs- that would give a 180 CrNC bond angle? Cr(NCS)63 undergoes substitution by ethylenediamine (en) according to the equation Cr(NCS)63+2enCr(NCS)2(en)2++4NCS Does Cr(NCS)2(en)2+ exhibit geometric isomerism? Does Cr(NCS)2(en)2+ exhibit optical isomerism?
Trimethylphosphine, P(CH3)3, can act as a ligand by donating the lone pair of electrons on the phosphorus atom. If trimethylphosphine is added to a solution of nickel(Il) chloride in acetone, a blue compound that has a molecular mass of approximately 270 g and contains 21.5% Ni, 26.0% Cl, and 52.5% P(CH3)3 can be isolated. This blue compound does not have any isomeric forms. What are the geometry and molecular formula of the blue compound?
The acetylacetone ion forms very stable complexes with many metallic ions. It acts as a bidentate ligand, coordi- nating to the metal at two adjacent positions. Suppose that one of the CH3 groups of the ligand is replaced by a CF; group, as shown here: н Trifluoromethyl acetylacetonate CF-Ç (ffac) C-CH3 :Ö: :0: Sketch all possible isomers for the complex with three tfac ligands on cobalt(III). (You can use the symbol to repre- sent the ligand.)
Which of these ligands can participate in linkage isomerism:(a) NO2-; (b) SO2; (c) NO3-? Explain with Lewis structures
. Show how the glycinate ion (H2N-CH2-COO-) can actas a bidentate ligand. (Draw a Lewis diagram if necessary.)Which atoms in the glycinate ion will bind to a metal ion?
3. Glycine has the structure NH;CH;COOH. It can lose aproton from the carboxyl group and form chelate ringsbonded through both the N and one of the O atoms. Draw structures for all possible isomers of tris(glycinato)cobalt(III). 4. Sketch structures of all isomers of M(AB)3, in which ABis a bidentate unsymmetrical ligand, and label the structuresfacor mer. 5. Sketch all isomers of the following. Indicate clearly eachpair of enantiomers. i. [PI(NH;);Cls]" ii. [Co(NH,);(H,O),CH]* iii. [Co(NH,):(H;0),BICI) iv. [CrH,O),BrCin v. [Pt(en):Cla)** vi. [Pt(bipy),BrC1}* How many possible isomers are there of an octahedral complex having the formula M(ABC)(NH,H;O)Br, where ABC is the tridentate ligand H,N-C,H,-PH-C,H-ASH2? How many of these consist of pairs of enantiomers? Sketch all isomers, showing clearly any pairs of enantiomers. The tridentate ligand may be abbreviated as N-P-As for simplicity.
1. Sketch all isomers of the following. Indicate clearly each pair of enantiomers. Multidentate ligands may be abbreviated as coordinating atoms bridged by a line. a) Cr(bipy)(H2O);BrF]* b) [Mn(en)(dppe)(xN-NO2)CI]¯
Consider the ligand of [Co(C₂O4)₂Cl₂]³¯; dichlorobisoxalatocobaltate(III) CI CI,, I. =c-o-co" C=0 =0 How many isomers can it have? What geometry does it have? Which of following is an appropriate counter ion?
Which one of the following formula/name pairs is incorrect? A. [Co(en):][Cr(CN)«], tris(ethylencdiamine)cobalt(III) hexacyanochromate(III) B. [Cr(en):][Co(CN)«], tris(ethylenediamine)chromium(III) hexacyanocobalate(III) C. [Pt(NH:)][PtCk], tetraammineplatinum(IV) hexachloroplatinate(II) D. [Pt(NH:).Clz][P!C1], tetraamminedichloroplatinum(II) tetrachloroplatinate(II) E. [Pt(NH3):CI][Pt(NH3)Cl;], triamminechloroplatinum(II) amminetrichloroplatinate(II)
Part C
oving to another question will save this response. complex [Co(NH3)6l absorbs light at a wavelength of 465 nm. What is the ligand field aplitting energy for the cormplez in Jlaole? 275 x 10 to negative x AMoving to another question will save this response.
CFT is applicable to molecules in geometries other than octahedral. In octahedral complexes, remember that the lobes of the eg set point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place,but now we have only four ligands located between the axes (as given). None of the orbitals points directly at the tetrahedral ligands. However, the eg set (along the Cartesian axes) overlaps with the ligands less than does the t2g set. By analogy with the octahedral case, predict the energy diagram for the d orbitals in a tetrahedral crystal field. To avoid confusion, the octahedral eg set becomes a tetrahedral e set, and the octahedral t2g set becomes a t2 set.