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- What is an absorption spectrum? If the absorption spectrum of a complex has just one band at 455 nm, what is the color of the complex?
Problem 1
Problem 3
What is the Lewis base in the reaction of oxalate with the mangenese ion to form [Mn(C2O4)3]2-? What is the oxidation state of Mn and the coordination number of the complex?
(a) Lewis base is C2O42-; Mn oxidation number is +3; coordination number is 3.
(b) Lewis base is C2O42-; Mn oxidination number is +2; coordination number is 6.
(c) Lewis base is Mn2+; Mn oxidation number is +2; coordination number is 3.
(d) Lewis base is Mn4+; Mn oxidation number is +4; coordination number is 6.
Problem 5
Refer to the figure showing the structure of various ligands to answer questions 4 and 5. Which ligand(s) can participate in linkage isomerism?
(a) All of the ligands can participate in linkage isomerism
(b) I, II, and III
(c) I and IV
(d) II and IV
- Arrange the following substances in order of increasing strength as oxidizing agents, and account for the trend: (a) Mn2+ (b) MnO2 (c) MnO4-.
Problem 6
Problem 7
Identify the false statement about the structures of the complex ion [Fe(en)2Cl2]+ shown below.
(a) Structures I and II are cis-trans isomers.
(b) Structures I and IV are cis-trans isomers.
(c) Structures I and III are enantiomers.
(d) Structures II and IV are enantiomers.
Problem 8.110c
Propose structures for molecules that meet the following
descriptions.
(c) Contains an S atom that has a coordinate covalent bond
- (b) What is the chemical formula of the third compound?
Problem 13
- In excess of NH3(aq), Zn2+ forms a complex ion, [Zn(NH3)4]2+ which has a formation constant Kf = 7.8 x 10^8. Calculate the concentration of Zn2+ in a solution prepared by adding 1.00 x 10^-2 mol Zn(NO3)2 to 1.00 L of 0.250 M NH3. (a) 7.9 x 10^-4 M (b) 2.8 x 10^-6 M (c) 3.9 x 10^-9 M (d) 6.4 x 10^-11 M
Problem 16
Problem 21.107
Draw a crystal field energy-level diagram, assign the electrons to orbitals, and predict the number of unpaired electrons for each of the following.
(a) [Cu(en)3]2+
(b) [FeF6]2-
(c) [Co(en)3]3+ (low spin)
Problem 21.64
What is the oxidation state of the metal in each of the complexes?
a. AgCl2–
b. [Cr(H2O)5Cl]2+
c. [Co(NCS)4]2–
d. [ZrF8]4–
e. [Fe(EDTA)(H2O)]–
Problem 21.2
Based on effective nuclear charge (Zeff), which ion is the strongest oxidizing agent?
(a) Cu2+
(b) Ni2+
(c) Fe2+
(d) Mn2+
Problem 21.133
The amount of paramagnetism for a first-series transition metal complex is related approximately to its spin-only magnetic moment. The spin-only value of the magnetic moment in units of Bohr magnetons (BM) is given by sqrt(n(n + 2)), where n is the number of unpaired electrons. Calculate the spin-only value of the magnetic moment for the 2+ ions of the first-series transition metals (except Sc) in octahedral complexes with (a) weak-field ligands and (b) strong-field ligands. For which electron configurations can the magnetic moment distinguish between high-spin and low-spin electron configurations?
Problem 21.54
What is the highest oxidation state for each of the elements from Sc to Zn?
Problem 21.29
The oxalate ion is a bidentate ligand as indicated in Figure 21.8. Would you expect the carbonate ion to be a monodentate or bidentate ligand? Explain your reasoning.
Problem 21.86
Which of the following complexes can exist as diastereoisomers?
(a) [Cr(NH3)2Cl4]-
(b) [Co(NH3)5Br]2+
(c) [MnCl2Br2]2- (tetrahedral)
(d) [Pt(NH3)2Br2]2-
Problem 21.1
What is the electron configuration of Co2+ and how many unpaired electrons are in the free transition metal ion?
(a) [Ar]3d54s2; 5 unpaired electrons
(b) [Ar]3d54s2; 1 unpaired electron
(c) [Ar]3d7; 3 unpaired electrons
(d) [Ar]3d7; 1 unpaired electron
Problem 21.95
The glycinate anion, gly-= NH2CH2CO2 -, bonds to metal ions through the N atom and one of the O atoms. Using to represent gly-, sketch the structures of the four stereoisomers of Co(gly)3.
Problem 21.96
Draw the structures of all possible diastereoisomers of an octahedral complex with the formula MA2B2C2. Which of the diastereoisomers, if any, can exist as enantiomers?
Problem 21.38
Predict the number of unpaired electrons for each of the following.
(c) Zn2+
(d) Cr3+
Problem 21.116
Although Cl- is a weak-field ligand and CN- is a strong field ligand, [CrCl6]3- and [Cr(CN)6]3- exhibit approximately the same amount of paramagnetism. Explain.
Problem 21.105
The [Cr(H2O)6]3+ ion is violet, and [Cr(CN)6]3- is yellow. Explain this difference using crystal field theory. Use the colors to order H2O and CN- in the spectrochemical series.
Problem 21.65
What is the oxidation state of the metal in each of the complexes?
a. [Ni(CN)5]3–
b. Ni(CO)4
c. [Co(en)2(H2O)Br]2+
d. [Cu(H2O)2(C2O4)2]2–
e. Co(NH3)3(NO2)3
Problem 21.121
Predict the crystal field energy-level diagram for a linear ML2 complex that has two ligands along the :
Problem 21.90
Draw all possible diastereoisomers of [Cr(C2O4)2(H2O)2]-. Which can exist as a pair of enantiomers?
Problem 21.102
Draw a crystal field energy-level diagram for the 3d orbitals of titanium in [Ti(H2O)6]3+]. Indicate the crystal field splitting, and explain why is [Ti(H2O)6]3+] colored.
Problem 21.9
What is the crystal field energy level diagram for the complex [Fe(NH3)6]3+?
(a)
(b)
(c)
(d)
Problem 21.93
What is a racemic mixture? Does it affect plane-polarized light? Explain.
Problem 21.6
What is the name of the compound [Fe(H2O)5(SCN)]Cl2?
(a) pentaaquathiocyanatoiron(III) chloride
(b) pentaaquachlorothiocyanato iron(III)
(c) pentaaquathiocyanatoiron(III) dichloride
(d) pentaaquathiocyanatoiron(II) chloride
Problem 21.114
Which of the following complexes are paramagnetic?
(a) [Mn(CN)6]3-
(b) [Zn(NH3)4]2+ (tetrahedral)
(c) [Fe(CN)6]4-
(d) [FeF6]4-
Problem 21.120
Look at the colors of the isomeric complexes in Figure 21.12, and predict which is the stronger field ligand, nitro (-NO2) of nitrito (-ONO). Explain.