?Sulfide \(\left(\mathrm{S}^{2-}\right)\) salts are notoriously insoluble in aqueous

When solid \(\mathrm{Cd}(\mathrm{OH})_{2}\) is added to a solution of 0.10 M NaI, some of it dissolves. Calculate the pH of the solution at equilibrium. Text Transcription: Cd(OH)_2

Two ligands, A and B, both form complexes with a particular metal ion. When the metal ion complexes with ligand A, the solution is green. When the metal ion complexes with ligand B, the solution is violet. Which of the two ligands results in the larger \(\Delta\) ? Text Transcription: Delta

Which element has the higher first ionization energy, Cu or Au?

The complexes of \(\mathrm{Fe}^{3+}\) have magnetic properties that depend on whether the ligands are strong or weak field. Explain why this observation supports the idea that electrons are lost from the 4s orbital before the 3d orbitals in the transition metals. Text Transcription: Fe^3+

Discuss these questions with the group and record your consensus answer. Have each group member choose a row of the transition metals in the periodic table and ask each to look up and graph (where appropriate) a trend, choosing from the following: electron configuration, atomic size, ionization energy, or electronegativity. Present your graph to the group. Describe the general trend and any notable exceptions. If possible, form new groups with individuals who researched the same property for a different row of the periodic table.

Discuss these questions with the group and record your consensus answer. Have each group member write down the names and formulas for two coordination compounds. Taking turns, show the formula to the group, and have the rest of the group members name the compound, with each member contributing one step in the process. Once each group member has had his or her formula named, repeat the process by showing only names to the group and having group members determine the correct formula.

Discuss these questions with the group and record your consensus answer. Working individually, draw a pair of coordination compounds that are isomers. Take turns showing your drawings to the group and having them identify the type of isomerism and the reasons that your drawing demonstrates that type of isomerism. If your group misidentifies your type of isomerism, rather than telling them the correct answer right away, point out the part of the structure that prevents it from being the type of isomerism they identified.

Discuss these questions with the group and record your consensus answer. Divide the electron configurations \(d^{1}\) through \(d^{10}\) among the group members such that every configuration is assigned to at least two group members. Working individually, draw the orbital diagram for the configurations assigned to you, including both high-spin and low-spin diagrams where possible. Present your diagrams to your group. Combine all diagrams into one set for the group. Text Transcription: d^1 d^10

Discuss these questions with the group and record your consensus answer. Working individually, review one of the applications of coordination complexes. Without you or your group members referring to the text, describe the application you reviewed without mentioning the key words in the heading of the subsection. As each group member describes the application they reviewed, take turns attempting to identify the key words from the heading of the subsection they are describing.

Many aqueous solutions of complex ions display brilliant colors that depend on the identities of the metal ion and ligand(s). Some ligands bind selectively to certain metal ions and produce a complex ion with characteristic colors. These distinctive complex ions serve as qualitative indicators of the presence of particular metal ions. For example, \(\mathrm{Fe}^{3+}\) is identified by the rapid formation of the intensely colored pentaaquathiocyanatoiron(III) complex ion, \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{SCN}\right]^{2+}\), when thiocyanate, \(\mathrm{SCN}^{-}\), is added to a solution containing hexaaquairon(III), \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\), according to the balanced chemical equation shown here: \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}(a q)+\mathrm{SCN}^{-}(a q) \rightleftharpoons\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{SCN}\right]^{2+}\) pale violet colorless intensely colored Examine the absorption spectrum of an aqueous solution of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{SCN}\right]^{2+}\) shown here and answer the questions. a. Based on the spectrum, what is the color of an \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{SCN}\right]^{2+}\) solution? b. Calculate the crystal field splitting energy,\(\Delta\), of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{SCN}\right]^{2+}\) in kJ/mol. c. The hexaaquairon(III) complex ion, \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\), produces a pale violet aqueous solution. Is the crystal field splitting energy, \(\Delta\), of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) smaller or larger than the \(\Delta\) of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{SCN}\right]^{2+}\)? d. On the basis of your answers to parts b and c, compare the crystal field strengths of water and thiocyanate ligands. e. The complex ion hexacyanoferrate(III), \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\), is red in aqueous solution. What can you conclude about the relative crystal field splitting energies of \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) and \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{SCN}\right]^{2+}\)? Text Transcription: Fe^3+ [Fe(H_2O)_5SCN]^2+ SCN^- [Fe(H_2O)_6]^3+ [Fe (H_2O)_6]^3+(aq) SCN^-(aq)rightleftharpoons[Fe(H_2O)_6]^3+ [Fe(CN)_6]^3- delta

Recall from Chapter 3 that Cr and Cu are exceptions to the normal orbital filling, resulting in a \([\mathrm{Ar}] 4 s^{1} 3 d^{x}\) configuration. Write the ground state electron configuration for each species. a. Cr, \(\mathrm{Cr}^{+}\), \(\mathrm{Cr}^{2+}\), \(\mathrm{Cr}^{3+}\) b. Cu, \(\mathrm{Cu}^{+}\), \(\mathrm{Cu}^{2+}\) Text Transcription: [Ar]4s^13d^x Cr^+ Cr^2+ Cr^3+ Cu^+ Cu^2+

Most of the second-row transition metals do not follow the normal orbital filling pattern. Five of them—Nb, Mo, Ru, Rh, and Ag—have a \([\mathrm{Kr}] 5 s^{1} 4 d^{x}\) configuration and Pd has a \([\mathrm{Kr}] 4 d^{10}\) configuration. Write the ground state electron configuration for each species. a. Mo, \(\mathrm{Mo}^{+}\), Ag, \(\mathrm{Ag}^{+}\) b. Ru, \(\mathrm{Ru}^{3+}\) c. Rh, \(\mathrm{Ru}^{2+}\) d. Pd, \(\mathrm{Pd}^{+}\), \(\mathrm{Pd}^{2+}\) Text Transcription: Mo^+ Ag^+ Ru^3+ Rh^2+ Pd^+ Pd^2+ [Kr]5s^14d^x [Kr] 4d^10

Draw the Lewis diagrams for each ligand. Indicate the lone pair(s) that may be donated to the metal. Indicate any you expect to be bidentate or polydentate. a. \(\mathrm{NH}_{3}\) b. \(\mathrm{SCN}^{-}\) c. \(\mathrm{H}_{2} \mathrm{O}\) Text Transcription: NH_3 SCN^- H_2O

Draw the Lewis diagrams for each ligand. Indicate the lone pair(s) that may be donated to the metal. Indicate any you expect to be bidentate or polydentate. a. \(\mathrm{CN}^{-}\) b. bipyridyl (bipy), which has the following structure: Text Transcription: CN^-

List all the different formulas for an octahedral complex made from a metal (M) and three different ligands (A, B, and C). Describe any isomers for each complex.

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. Draw all the possible isomers of: a. square planar \(\left[\mathrm{Ni}(\mathrm{gly})_{2}\right]\) b. tetrahedral \(\left[\mathrm{Zn}(\mathrm{gly})_{2}\right]\) c. octahedral \(\left[\mathrm{Fe}(\mathrm{gly})_{3}\right]\) Text Transcription: [Ni(gly)_2] Zn(gly)_2] [Fe(gly)_3]

Oxalic acid solutions remove rust stains. Draw a complex ion that is likely responsible for this effect. Does it have any isomers?

W, X, Y, and Z are different monodentate ligands. a. Is the square planar \([\mathrm{NiWXYZ}]^{2+}\) optically active? b. Is the tetrahedral \([\mathrm{ZnWXYZ}]^{2+}\) optically active? Text Transcription: [NiWXYZ]^2+ [ZnWXYZ]^2+

Hexacyanomanganate(III) ion is a low-spin complex. Draw the crystal field splitting diagram with electrons filled in appropriately. Is this complex paramagnetic or diamagnetic?

Determine the color and approximate wavelength absorbed most strongly by each solution. a. blue solution b. red solution c. yellow solution

Draw the structures of all the geometric isomers of \(\left[\mathrm{Ru}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right.\left.\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]^{+}\). Draw the mirror images of any that are chiral. Text Transcription: [Ru(H_2O)_2(NH_3)2Cl_2]^+

A 0.32 mol amount of \(\mathrm{NH}_{3}\) is dissolved in 0.47 L of a 0.38 M silver nitrate solution. Calculate the equilibrium concentrations of all species in the solution. Text Transcription: NH_3

When a solution of \(\mathrm{PtCl}_{2}\) reacts with the ligand trimethylphosphine, \(\mathrm{P}\left(\mathrm{CH}_{3}\right)_{3}\), two compounds are produced. The compounds share the same elemental analysis: 46.7% Pt; 17.0% Cl; 14.8% P; 17.2% C; 4.34% H. Determine the formula, draw the structure, and give the systematic name for each compound. Text Transcription: P(CH_3)_3 PtCl_2

Draw a crystal field splitting diagram for a trigonal planar complex ion. Assume the plane of the molecule is perpendicular to the z axis.

Draw a crystal field splitting diagram for a trigonal bipyramidal complex ion. Assume the axial positions are on the z axis.

Explain why \(\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) is paramagnetic, while \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) is diamagnetic. Text Transcription: [Ni(NH_3)_4^]2+ [Ni(CN)_4]^2-

Sulfide \(\left(\mathrm{S}^{2-}\right)\) salts are notoriously insoluble in aqueous solution. a. Calculate the molar solubility of nickel(II) sulfide in water. \(K_{\mathrm{sp}}(\mathrm{NiS})=3 \times 10^{-16}\) b. Nickel(II) ions form a complex ion in the presence of ammonia with a formation constant \(\left(K_{f}\right)\) of \(2.0 \times 10^{8}\): \(\mathrm{Ni}^{2+}+6 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\). Calculate the molar solubility of NiS in \(3.0 \ \mathrm{M} \ \mathrm{NH}_{3}\). c. Explain any differences between the answers to parts a and b. Text Transcription: (S^2-) K_sp(NiS) = 3 x 10^-16 (K_f) 2.0 x 10^8 Ni^2+ + 6 NH_3 rightleftharpoons [Ni(NH_3)_6]^2+ 3.0 M NH_3

Calculate the solubility of \(\mathrm{Zn}(\mathrm{OH})_{2}(\mathrm{~s})\) in 2.0 M NaOH solution. (Hint: You must take into account the formation of \(\mathrm{Zn}(\mathrm{OH})_{4}{ }^{2-}\), which has a \(K_{f}=2 \times 10^{15}\).) Text Transcription: Zn(OH)_2(s) Zn(OH)_4^2- K_f = 2 x 10^15

Halide complexes of metal M of the form \(\left[\mathrm{MX}_{6}\right]^{3-}\) are found to be stable in aqueous solution. But it is possible that they undergo rapid ligand exchange with water (or other ligands) that is not detectable because the complexes are less stable. This property is referred to as their lability. Suggest an experiment to measure the lability of these complexes that does not employ radioactive labels. Text Transcription: [MX_6]^3-

The \(K_{f}\) for \(\left[\mathrm{Cu}(\mathrm{en})_{2}\right]^{2+}\) is much larger than the one for \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\). This difference is primarily an entropy effect. Explain why and calculate the difference between the \(\Delta S^{\circ}\) values at 298 K for the complete dissociation of the two complex ions. (Hint: The value of \(\Delta H\) is about the same for both systems.) Text Transcription: K_f deltaS degree deltaH [Cu(en)_2]^2+ [Cu(NH_3)_4]^2+

When a transition metal atom forms an ion, which electrons are lost first?

Explain why transition metals exhibit multiple oxidation states instead of a single oxidation state (which most of the main-group metals do).

Why is the +2 oxidation state so common for transition metals?

Explain why atomic radii of elements in the third row of the transition metals are no larger than those of elements in the second row.

Gold is the most electronegative transition metal. Explain.

Briefly define each term. a. coordination number b. ligand c. bidentate and polydentate d. complex ion e. chelating agent

Using the Lewis acid–base definition, how would you categorize a ligand? How would you categorize a transition metal ion?

Explain the differences between each pair of isomer types. a. structural isomer and stereoisomer b. linkage isomer and coordination isomer c. geometric isomer and optical isomer

Which complex ion geometry has the potential to exhibit cis–trans isomerism: linear, tetrahedral, square planar, octahedral?

How can you tell whether a complex ion is optically active?

Explain the differences between weak-field and strong-field metal complexes.

Explain why compounds of \(\mathrm{Sc}^{3+}\) are colorless, but compounds of \(\mathrm{Ti}^{3+}\) are colored. Text Transcription: Sc^3+ Ti^3+

Explain why compounds of \(\mathrm{Zn}^{2+}\) are white, but compounds of \(\mathrm{Cu}^{2+}\) are often blue or green. Text Transcription: Zn^2+ Cu^2+

Explain the differences between high-spin and low-spin metal complexes.

Why are almost all tetrahedral complexes high-spin?

Many transition metal compounds are colored. How does crystal field theory account for this?

Write the ground state electron configuration for each atom and ion pair a. Ni, \(\mathrm{Ni}^{2+}\) b. Mn, \(\mathrm{Mn}^{4+}\) c. Y, \(\mathrm{Y}^{+}\) d. Ta, \(\mathrm{Ta}^{2+}\) Text Transcription: Ni^2+ Mn^4+ Ta^2+

Write the ground state electron configuration for each atom and ion pair. a. Zr, \(\mathrm{Zr}^{2+}\) b. Co, \(\mathrm{Co}^{2+}\) c. Tc, \(\mathrm{Tc}^{3+}\) d. Os, \(\mathrm{Os}^{4+}\) Text Transcription: Zr^2+ Co^2+ Tc^3+ Os^4+

Determine the highest possible oxidation state for each element. a. V b. Re c. Pd

Which first-row transition metal(s) has the following highest possible oxidation state? a. +3 b. +7 c. +4

Determine the oxidation state and coordination number of the metal ion in each complex ion. a. \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) b. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right]^{-}\) c. \(\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]^{2-}\) d. \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}\) Text Transcription: [Cr(H_2O)_6]^3+ [Co(NH_3)_3Cl3]^- [Cu(CN)_4]^2- [Ag(NH_3_2]^+

Determine the oxidation state and coordination number of the metal ion in each complex ion. a. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Br}\right]^{2+}\) b. \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}\) c. \(\left[\operatorname{Co}(o x)_{3}\right]^{4}\) d. \(\left[\mathrm{PdCl}_{4}\right]^{2-}\) Text Transcription: a. [Co(NH_3)5Br]^2+ b. [Fe(CN)_6]^4- c. [Co(ox)_3]^4- d. [PdCl_4]^2-

Name each complex ion or coordination compound. a. [Cr(H2O)6]3+ b. [Cu(CN)4]2- c. [Fe(NH3)5Br]SO4 d. [Co(H2O)4(NH3)(OH)]Cl2

Name each complex ion or coordination compound. a. \(\left[\mathrm{Cu}(\mathrm{en})_{2}\right]^{2+}\) b. \(\left[\mathrm{Mn}(\mathrm{CO})_{3}\left(\mathrm{NO}_{2}\right)_{3}\right]^{2+}\) c. \(\mathrm{Na}\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\mathrm{ox})_{2}\right]\) d. \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) Text Transcription: a. [Cu(en)_2]^2+ b. [Mn(CO_)3(NO_2)_3]^2+ c. Na[Cr(H_2O)_2(ox)_2] d. [Co(en)_3][Fe(CN)_6]

Write the formula for each complex ion or coordination compound. a. hexaamminechromium(III) b. potassium hexacyanoferrate(III) c. ethylenediaminedithiocyanatocopper(II) d. tetraaquaplatinum(II) hexachloroplatinate(IV)

Write the formula for each complex ion or coordination compound. a. hexaaquanickel(II) chloride b. pentacarbonylchloromanganese(I) c. ammonium diaquatetrabromovanadate(III) d. tris(ethylenediamine)cobalt(III) trioxalatoferrate(III)

Write the formula and the name of each complex ion. a. a complex ion with \(\mathrm{Co}^{3+}\) as the central ion and three \(\mathrm{NH}_{3}\) molecules and three \(\mathrm{CN}^{-}\) ions as ligands b. a complex ion with \(\mathrm{Cr}^{3+}\) as the central ion and a coordination number of 6 with ethylenediamine ligands Text Transcription: Co^3+ NH_3 CN^- Cr^3+

Write the formula and the name of each complex ion or coordination compound. a. a complex ion with four water molecules and two \(\mathrm{ONO}^{-}\) ions connected to an iron(III) ion b. a coordination compound made of two complex ions: one a complex of vanadium(III) with two ethylenediamine molecules and two \(\mathrm{Cl}^{-}\) ions as ligands and the other a complex of nickel(II) having a coordination number of 4 with \(\mathrm{Cl}^{-}\) ions as ligands Text Transcription: ONO^- Cl^- Cl^-

Draw two linkage isomers of \(\left[\operatorname{Mn}\left(\mathrm{NH}_{3}\right)_{y}\left(\mathrm{NO}_{2}\right)\right]^{2+}\). Text Transcription: [Mn(NH_3)_5(NO_2)]^2+

Draw two linkage isomers of \(\left[\mathrm{PtCl}_{3}(\mathrm{SCN})\right]^{2-}\). Text Transcription: [PtCl_3(SCN)]^2-

Write the formulas and names for the coordination isomers of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}\). Text Transcription: [Fe(H_2O)_6]Cl_2

Write the formulas and names for the coordination isomers of \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]\left[\mathrm{Cr}(\mathrm{ox})_{3}\right]\). Text Transcription: [Co(en)_3] [Cr(ox)_3]

Which complexes exhibit geometric isomerism? a. \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{5}(\mathrm{OH})\right]^{2+}\) b. \(\left[\mathrm{Cr}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]^{+}\) c. \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{2}\right]^{+}\) d. \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right) \mathrm{Cl}_{3}\right]^{-}\) e. \(\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\mathrm{CN})_{2}\right]\) Text Transcription: [Cr(NH_3)_5(OH)]^2+ [Cr(en)_2Cl_2]^+ [Cr(H_2O)(NH_3)_3Cl_2]^+ [Pt(NH_3)Cl_3]^- [Pt(H_2O)_2(CN)_2]

Which complexes exhibit geometric isomerism? a. \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\mathrm{ox})_{2}\right]^{-}\) b. \(\left[\operatorname{Co}(\mathrm{en})_{3}\right]^{3+}\) c. \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{OX})\right]^{+}\) d. \(\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{en})\right]^{2+}\) e. \(\left[\mathrm{Ni}(\mathrm{CO})_{2} \mathrm{Cl}_{2}\right]\) Text Transcription: [Co(H_2O)_2(ox)_2]^- [Co(en)_3]^3+ [Co(H_2O)_2(NH_3)_2(ox)]^+ [Ni(NH_3)_2(en)]^2+ [Ni(CO)_2Cl_2]

If W, X, Y, and Z are different monodentate ligands, how many geometric isomers are there for each ion? a. square planar \([\mathrm{NiWXYZ}]^{2+}\) b. tetrahedral \([\mathrm{ZnWXYZ}]^{2+}\) Text Transcription: [NiWXYZ]^2+ [ZnWXYZ]^2+

How many geometric isomers are there for each species? a. \(\left[\mathrm{Fe}(\mathrm{CO})_{3} \mathrm{Cl}_{3}\right]\) b. \(\left[\mathrm{Mn}(\mathrm{CO})_{2} \mathrm{Cl}_{2} \mathrm{Br}_{2}\right]^{+}\) Text Transcription: [Fe(CO)_3Cl_3] [Mn(CO)_2Cl_2Br_2]^+

Draw the structures and label the type for all the isomers of each ion. a. \(\left[\mathrm{Cr}(\mathrm{CO})_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]^{3+}\) b. \(\left[\mathrm{Pd}(\mathrm{CO})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}\right]^{+}\) Text Transcription: [Cr(CO)_3(NH_3)_3]^3+ [Pd(CO)_2(H_2O)Cl]^+

Draw the structures and label the type for all the isomers of each species. a. \(\left[\mathrm{Fe}(\mathrm{CO})_{4} \mathrm{Cl}_{2}\right]^{+}\) b. \(\left[\mathrm{Pt}(\mathrm{en}) \mathrm{Cl}_{2}\right]\) Text Transcription: Fe(CO)_4Cl_2]^+ [Pt(en)Cl_2]

Determine if either isomer of \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{OX})_{2}\right]^{-}\) is optically active. Text Transcription: [Cr(NH_3)_2(ox)_2]-

Determine if either isomer of \(\left[\mathrm{Fe}(\mathrm{CO})_{3} \mathrm{Cl}_{3}\right]\) is optically active. Text Transcription: [Fe(CO)_3Cl_3]

Draw the octahedral crystal field splitting diagram for each metal ion. a. \(\mathrm{Zn}^{2+}\) b. \(\mathrm{Fe}^{3+}\) (high- and low-spin) c. \(\mathrm{V}^{3+}\) d. \(\mathrm{Co}^{2+}\) (high-spin) Text Transcription: Zn^2+ Fe^3+ V^3+ Co^2+

Draw the octahedral crystal field splitting diagram for each metal ion. a. \(\mathrm{Cr}^{3+}\) b. \(\mathrm{Cu}^{2+}\) c. \(\mathrm{Mn}^{3+}\) (high- and low-spin) d. \(\mathrm{Fe}^{2+}\) (low-spin) Text Transcription: Cr^3+ Cu^2+ Mn^3+ Fe^2+

The \(\left[\mathrm{CrCl}_{6}\right]^{3-}\) ion has a maximum absorbance in its absorption spectrum at 735 nm. Calculate the crystal field splitting energy (in kJ>mol) for this ion. Text Transcription: [CrCl_6]^3-

The absorption spectrum of the complex ion \(\left[\mathrm{Rh}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) has maximum absorbance at 295 nm. Calculate the crystal field splitting energy (in kJ>mol) for this ion. Text Transcription: [Rh(NH_3)_6]^3+

Three complex ions of cobalt(III), \(\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}\), \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\), and \(\left[\mathrm{CoF}_{6}\right]^{3-}\), absorb light at wavelengths of (in no particular order) 290 nm, 440 nm, and 770 nm. Match each complex ion to the appropriate wavelength absorbed. What color would you expect each solution to be? Text Transcription: [Co(CN)_6]^3- [Co(NH_3)_6]^3+ [CoF_6]^3-

Three bottles of aqueous solutions are discovered in an abandoned lab. The solutions are green, yellow, and purple. It is known that three complex ions of chromium(III) were commonly used in that lab: \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\), \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\), and \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4} \mathrm{Cl}_{2}\right]^{+}\). Determine the likely identity of each of the colored solutions. Text Transcription: [Cr(H_2O)_6]^3+ [Cr(NH_3)_6]^3+ [Cr(H2O)_4Cl_2]^+

The \(\left[\mathrm{Mn}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) ion is paramagnetic with five unpaired electrons. The \(\mathrm{NH}_{3}\) ligand is usually a strong-field ligand. Is \(\mathrm{NH}_{3}\) acting as a strong-field in this case? Text Transcription: [Mn(NH_3)_6]^2+ NH_3 NH_3

The complex \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) is paramagnetic. Is the \(\mathrm{H}_{2} \mathrm{O}\) ligand inducing a strong or weak field? Text Transcription: [Fe(H_2O)_6]^2+ H_2O H_2O

How many unpaired electrons do you expect each complex ion to have? a. \(\left[\mathrm{RhCl}_{6}\right]^{3-}\) b. \(\left[\mathrm{Co}(\mathrm{OH})_{6}\right]^{4-}\) c. \(\text { cis- }\left[\mathrm{Fe}(\mathrm{en})_{2}\left(\mathrm{NO}_{2}\right)_{2}\right]^{+}\) Text Transcription: [RhCl_6]^3- [Co(OH)_6]^4- cis-[Fe(en)_2(NO_2)_2]^+

How many unpaired electrons do you expect each complex ion to have? a. \(\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{4}\) b. \(\left[\mathrm{MnF}_{6}\right]^{4-}\) c. \(\left[\mathrm{Ru}(\mathrm{en})_{3}\right]^{2+}\) Text Transcription: [Cr(CN)_6]^4- [MnF_6]^4- [Ru(en)_3]^2+

How many unpaired electrons do you expect the complex ion \(\left[\mathrm{CoCl}_{4}\right]^{2-}\) to have if it is a tetrahedral shape? Text Transcription: [CoCl_4]^2-

The complex ion \(\left[\mathrm{PdCl}_{4}\right]^{2-}\) is known to be diamagnetic. Use this information to determine if it is a tetrahedral or square planar structure. Text Transcription: [PdCl_4]^2-

What structural features do hemoglobin, cytochrome c, and chlorophyll have in common?

Identify the central metal atom in each complex. a. hemoglobin b. carbonic anhydrase c. chlorophyll d. iron blue

Hemoglobin exists in two predominant forms in our bodies. One form, known as oxyhemoglobin, has \(\mathrm{O}_{2}\) bound to the iron and the other, known as deoxyhemoglobin, has a water molecule bound instead. Oxyhemoglobin is a low-spin complex that gives arterial blood its red color, and deoxyhemoglobin is a high-spin complex that gives venous blood its darker color. Explain these observations in terms of crystal field splitting. Would you categorize \(\mathrm{O}_{2}\) as a strong- or weak-field ligand? Text Transcription: O_2 O_2

Carbon monoxide and the cyanide ion are both toxic because they bind more strongly than oxygen to the iron in hemoglobin (Hb). \(\mathrm{Hb}+\mathrm{O}_{2} \rightleftharpoons \mathrm{HbO}_{2}\) \(K=2 \times 10^{12}\) \(\mathrm{Hb}+\mathrm{CO} \rightleftharpoons \mathrm{HbCO}\) \(K=1 \times 10^{14}\) Calculate the equilibrium constant value for this reaction. \(\mathrm{HbO}_{2}+\mathrm{CO} \rightleftharpoons \mathrm{HbCO}+\mathrm{O}_{2}\) Does the equilibrium favor reactants or products? Text Transcription: Hb + O_2 rightleftharpoons HbO_2 K = 2 x 10^12 Hb + CO rightleftharpoons HBCO K = 1 x 10^14 HbO_2 + CO rightleftharpoons HbCO + O