(a) Predict whether the glycinate ion, H2N-CH COO is a monodentate, bidentate, or tridentate ligand: monodentate bidentate O tridentate (b) What experiment could you perform to test this prediction? Dissolve a complex solid containing this ligand in water and measure how many ions are produced. Compare the color of a metal complex containing this ligand with that of the same metal bound to a monodentate, bidentate, or tridentate ligand. Perform a ligand substitution reaction to determine the stoichiometric ratio between this ligand and a metal that forms an octahedral complex. Look up the answer on Google. Determine the number of unpaired electrons in a metal-complex containing this ligand using a magnetic susceptibility balance.

(a) Predict whether the glycinate ion, H2N-CH COO is a monodentate, bidentate, or tridentate ligand: monodentate bidentate O tridentate (b) What experiment could you perform to test this prediction? Dissolve a complex solid containing this ligand in water and measure how many ions are produced. Compare the color of a metal complex containing this ligand with that of the same metal bound to a monodentate, bidentate, or tridentate ligand. Perform a ligand substitution reaction to determine the stoichiometric ratio between this ligand and a metal that forms an octahedral complex. Look up the answer on Google. Determine the number of unpaired electrons in a metal-complex containing this ligand using a magnetic susceptibility balance.

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

Dimethyldithiocarbamate (abbreviated as dmdtc) is an anionic bidentate ligand with a chemical formula (S2CNMe2)- - where Me stands for methyl group (-CH3). In the photo above, this ligand coordinates to a metal through its 2 sulfur atoms (where M represents a metal). When three dmdtc ligands bind to a ferric ion (Fe3+), a stable coordination complex called ferbam is formed. Given this information, answer / identify the following. complex geometry hybridization type of the central atom coordination number
Name the following metal complexes or complex ions: formula name [Fe(OH), (en),] [V(CN),(NH,).] TiF ?
Be sure to answer all parts. Complete the following statements for the complex ion [Co(en)2(H2O)CN]2+. (a) en is the abbreviation for (b) The oxidation number of Co is (c) The coordination number of Co is (d) is a bidentate ligand. (en) Co(en)2 CN H2O
Draw the crystal field diagram of [W(CO)6]. Determine the (a) Electronic configuration in terms t2geg (b) Number of unpaired electrons (c) Ligand field stabilization energy in terms of ΔO or ΔT
Q4/ geometrical isomerism is found in square planar and octahedral complexes but not found in tetrahedral complexes? Q5/ Which of the following can function as a bidentate ligand? NH₁, CO, CO, OH
Make a prediction about each structures' splitting energy relative to an octahedral complex with all water ligands. Provide some theoretical basis for these claims (see the protocol for Part 2 and textbook chapter 22 to deepen understanding of these concepts). the structure is K3[Fe(C2O4)3]· 2 H2O
Consider the coordination complex with the formula: [Fe(NH3)4(NO2)2]Br a. Can this complex have isomers? If so state which types? Explain your decisions about isomers based on the number and type of each ligand. Hint: what atoms of NO2 - ion can bind the metal ion? Also do you have ‘looping’ ligands? Isomer types include: geometric (cis-trans), linkage, optical, and coordination. b. Draw the crystal field diagram (of d orbital energies) for this complex. State the number of unpaired electrons on the Fe ion. Label the potential energy axis and the 2 orbital levels on your diagram. c. Predict the color of this complex. Explain your answer based on the field strength of the two types of ligands in the complex, using field strength listing below and the color wheel provided on the equations page. d. Will this complex be paramagnetic or diamagnetic? Explain your decision briefly based on the number of unpaired electrons on the metal ion in the complex.
ose the false statement about isomerism in metal complexes. a) Enantiomers are non-superimposable mirror images, cis and trans isomers rotate the plane of polarization of plane-polarized light. c) it is possible for an octahedral coordination compound of formula M(NH3)5CIBr to have ionization isomers, aka coordination isomers. Linkage isomerism can occur in complexes with nitrite (NO2-) as a ligand. tion 14 ch of the following properties differ i
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
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).
The color for each “hexaaqua” complex is given below. Select the ligands thatcould change the color of the complex to the color in column 2.Hint: The spectrochemical Series will come in handy here.I− < Br− < Cl− < F− < OH− < H2O < SCN− < NH3 < en < NO2− < CN− < CO
Cobalt(III) has a coordination number of 6 in all its complexes. Is the carbonate ion amonodentate or bidentate ligand in the [Co(NH3)4(CO3)] + ion?